QD 


UNIVERSITY  OF  CALIFORNIA  PUBLICATIONS 
IN 

PHYSIOLOGY 

Vol.  5,  No.  4,  pp.  23-69  March  29,  1919 


TABLE  OF  PH,  H+  AND  OH~  VALUES  CORRE- 
SPONDING TO  ELECTROMOTIVE  FORCES 
DETERMINED  IN  HYDROGEN  ELECTRODE 
MEASUREMENTS,  WITH  A  BIBLIOGRAPHY. 


! 

CARL  L.  A.j  SCHMIDT  AND  D.  R.  HOAGLAND 


UNIVERSITY  OF  CALIFORNIA  PRESS 
BERKELEY 


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'...*  Voi/S/  •  J."  JCJie/ Control  of  Heliotropic  Eeactions  in  Fresh-water  Crustaceans  by 

Chemicals,    especially    CO3    (a    preliminary    communication),    by 

;•:*•;*•.".  ^     •  .«3acqijes  Loeb.    Pp.  1-S.    November,  1904. .05 

*T  .**!•.•  *1  ta^vftffcHsr  Experiments  on  Heterogeneous  Hybridization  in  Eehinoderma, 

by  Jacques  Loeb,    Pp.  5-30.    December,  1904 
8.  Influence  of  Calcium  and  Barium  on  the  Secretory  Activity  of  tha 

Kidneys    (second    communication),    by    John    Bruce    MacCallum, 

Pp.  31-42.    December,  1904. 

4.  Note    on    the    Gaivanotropie    Eeactions    of    the    Medusa    Polyorchis 

penicillata  A,  Agassiz,  by  Frank  W.  Bancroft.    Pp.  43-46,    Decem- 
ber, 1904. 
Nos.  2,  S  and  4  in  one  cover —      .48 

5.  The  Action  on  the  Intestines  of  Solutions  containing  two  Salts,  by 

John  Bruce  MacCallum.    Pp.  47-64.    January,  1905. 

6.  The  Action   of  Purgatives  in   a  Crustacean    (Sida   crystalline'),   by 

John  Bruce  MacCallum.    Pp.  65-70.    January,  1905. 
Nos.  5  and  6  in  one  cover .26 

7.  On  the  Validity  of  Pfluger's  Law  for  the  Galvanic  Action  of  Para- 

mecium    (preliminary    communication),    by    Frank    W.    Bancroft. 
P.  71.    February,  1905. 

8.  "On   Fertilization,   Artificial   Parthenogenesis   and   Cytolysis    of   the 

Sea  urchin  Egg,  by  Jacques  Loeb.  Pp.  73-81.    February,  1905. 
Nos.  7  and  8  in  one  cover 15 

9.  On  an  Improved  Method  of  Artificial  Parthenogenesis,  by  Jacques 

Loeb.    Pp.  83-86.     February,  1905... .05 

10.  On  the  Diuretic  Action  of  Certain  Haemolytics,  and  the  Action  of 

Calcium  in  Suppressing  Haemoglobinuria  (preliminary  communica- 
tion), by  John  Bruce  MacCallum.    Pp.  87-88.    March,  1905. 

11.  On  an  Improved  Method  of  Artificial -Parthenogenesis  (second  com- 

munication), by  Jacques  Loeb.    Pp.  89-92.    March,  1905. 
Nos.  10  and  11  in  one  cover .^- 05 

12.  The  Diuretic  Action  of  Certain  Haemolytics  and  the  Influence  of 

Calcium  and  Magnesium  in  Suppressing  the  Haemolysis    (second 
communication),  by  John  Bruce  MacCallum,  Pp.  93-103.  May,  1905. 
18.  The  Action  of  Pilocarpine  and  Atropin  on  the  Flew  of  Urina,  by 
John  Bruce  MacCallura.    Pp.  105  112.    May,  1905. 
Nos.  12  and  13  in  one  cover .28 

14.  On  an  Improved  Method  of  Artificial  Parthenogenesis   (third  com- 

munication), by  Jacques  Loeb.    Pp.  113-128.    May,  1905 _      .18 

15.  On  the   Influence   of  Temperature   upon   Cardiac   Contractions   and 

its  Eolation  to  Influence  of  Temperature  upon  Chemical  Eeaction 
Velocity,  by  Charles  D,  Snyder.    Pp.  125-146.    September.  1905 26 

16.  Artificial  Membrane  Formation  and  Chemical  Fertilization  in  a  Star- 

fish (Astet-ina).,  by  Jacques  Loeb,    Pp.  147-158.    September,  1905 15 

17.  On  the  Influence  of  Electrolytes  upon  the  Toxicity  of  Alkaloids  (pre- 

liminary communication),  by  T.  Brailsford  Eobertson.    Pp.  159-162. 
October,  1905 _~ -      .05 

18.  Studies    on    the    Toxicity    of    Sea-water    for    Fresh- water    Animal* 

(Gammarus   pulex  De   Geer),   by   C.   H.   Wolfgang   Ostwald.     Pp. 
163-191;  plates  1-6.     November,  1905 85 

19.  On  the  Validity  of  Pfltiger's  Law  for  the  Galvanotropic  Eeactions 

of  Paranieciuia,  by  Frank  W.  Bancroft.    Pp.  193-215;  8  text  figures. 

November,   1905 20 

Vol.8,      1.  On   Chemical   Methods   by  which   the   Eggs   of   &  Mollusc    (Lottia 
Gigantea)    can   ba   caused  to   become   Mature,   by   Jacques  Loeb. 

Pp.  1-8.    November,  1905 05 

2.  On  the  Changes  In  the  Nerve  and  Muscle  which  ssem  to  Underlie  the 
Electrotonic  Effect  of  the  Galvanic  Current,  by  Jacques  Loeb.  Pp. 
9-15.  December,  1905 ~ 05 


UNIVERSITY  OF  CALIFORNIA   PUBLICATIONS 

IN 

PHYSIOLOGY 

Vol.  5,  No.  4,  pp.  23-69  March  29,  1919 


TABLE  OF  PH,  H+  AND  OH"  VALUES  CORRE- 
SPONDING TO  ELECTROMOTIVE  FORCES 
DETERMINED  IN  HYDROGEN  ELECTRODE 
MEASUREMENTS,  WITH  A  BIBLIOGRAPHY.* 

BY 

GAEL  L.  A.  SCHMIDT  AND  D.  E.  HOAGLAND 

(From  the   Hearst  Laboratory   of  Pathology   and  Bacteriology,   the   Department 

of  Biochemistry,  and  the  Division  of  Agricultural  Chemistry  of  the 

University  of  California.) 


The  importance  of  measurements  of  reaction  or  hydrogen  ion 
concentration  is  well  recognized  in  many  fields  of  scientific  work.  In 
biological  studies  the  reaction  of  the  body  tissues  and  fluids,  optimum 
reaction  for  enzymes,  and  the  dissociation  of  the  proteins  are  among 
the  many  subjects  investigated.  Recent  work  has  shown  the  impor- 
tance of  the  reaction  of  the  media  for  the  proper  growth  of  micro- 
organisms, and  in  the  field  of  agricultural  chemistry  the  relation  of 
the  acidity  of  the  soil  to  the  growth  of  the  plant  has  also  been  indi- 
cated. The  extensive  application  of  the  electrometric  method  for 
determining  hydrogen  ion  concentration  has  led  to  its  use  in  labora- 
tories without  extensive  equipment,  and  where  the  extreme  accuracy 
so  necessary  to  the  theoretical  chemist  is  less  essential  than  the  ability 
quickly  to  carry  out  a  large  number  of  determinations  without  the 
use  of  refined  apparatus.  The  results  so  obtained  may  still  have  an 
accuracy  well  within  the  limits  of  interpretation. 

With  a  view  of  facilitating  measurements  of  hydrogen  ion  concen- 
tration, one  of  us  (Schmidt)37  some  years  ago  prepared  tables  for  the 
conversion  of  voltages  into  hydrogen  or  hydroxyl  ion  concentrations, 
thus  rendering  unnecessary  the  somewhat  tedious  computations.  Since 

*  Aided  in  part  by  a  grant  from  the  George  Williams  Hooper  Foundation  for 
Medical  Eesearch. 


821905 


"24  University  of  California  Publications  in  Physiology      [VOL.  5 

then  Sorensen's  suggestion  of  using  PH*  as  a  measure  of  reaction 

instead  of  hydrogen  ion  concentration  has  been  quite  generally  adopted 

and  the  expression  of  results  simplified.    For  many  purposes,  however, 

.  both  units  are  desirable.     McClendon172  has  published  a  chart  from 

"*.•>•*       .»  '.wllifefi;  both  of  the  above  values  within  a  certain  range  can  be  read. 

*:  ;";"'/Th;e  coujtinited  demand  for,  as  well  as  the  advantages  possessed  by  a 
direct  'conversion  table  led  us  to  recalculate  the  former  tables  and 
include  also  the  PH  values  for  both  the  normal  and  N/10  KCl-calomel 
electrode.  For  a  range  of  voltages  not  frequently  used  the  calculations 
have  been  made,  as  in  the  former  tables,  for  every  two  millivolts,  while 
for  a  certain  range  on  either  side  of  the  neutral  point  this  has  been 
done  for  each  millivolt. 

We  have  also  included  an  extensive  bibliography,  somewhat  arbi- 
trarily classified,  since  it  is  quite  impossible  to  arrange  the  references 
according  to  the  subjects  treated  without  either  duplicate  citation  or 
cross-indexing.  While  many  of  the  references  given  possess  merely 
historical  interest,  they  have  nevertheless  been  included  and  are  of 
value  as  showing  to  what  extent  certain  fields  have  been  investigated. 
We  have  cited  only  those  references  which  include  determinations  of 
hydrogen  ion  concentration  by  the  electrometrie  method,  by  indicators, 
or  by  the  use  of  buffer  mixtures.  Certain  other  references  appertain- 
ing to  the  theory  of  the  hydrogen  electrode  or  methods  of  measuring 
electromotive  forces  have  also  been  included. 

Our  calculations  are  based  on  the  recent  measurements  by  Lewis, 
Brighton,  and  Sebastian61  of  the  potential  of  the  normal  and  N/10  KCl- 
calomel  electrodes  and  the  dissociation  constant  of  water.  For  the 
potential  of  the  normal  calomel  electrode,  referred  to  the  potential 
of  the  normal  hydrogen  electrode  as  zero,  we  have  taken 

H2,H+  (M)  ||  Hg,  HgCl,  KC1  (M)  ;  E  =  0.283  volt 


*  The  term  PH  is  given  to  the  exponent  of  10  taken  as  a  positive  number.     This 
is  the  most  rational  system  since  all  values  are  expressed  in  the  same  units.     Thus 
CH  =  5.03  X  10"10  can  be  expressed  entirely  as  a  power  of  10. 
5.03  =  10°-702  (since  Iog10  5.03  =  0.702) 

CH  =  10°-702  X  10-10 
_3  Q-9.298 

PH  — 9.298 
Another  example :  To  find  PH,  when  CH  =  0.409  X  10'7 

PH  =  log10     05 

PH  =  Iog10 1  —  Iog10  CH 

Log10  CH  =  10-7  X  lO1-™ 

=  8.612 

PH  =  17.388  — 10 
PH  =  7.388 


Schmidt-Hoagland:  Table  of  PH,  H+  and  OH-  Values          25 

and  for  the  difference  in  potential  between  the  normal  and  N/10  KC1- 
calomel  electrodes 

Hg,  HgCl,  KC1  (0.1  M)  ||  HgCl,  KC1,  (M)  ;  E  =  0.053. 

This  gives  a  value  of  0.336  volt  for  the  N/10  KCl-calomel  electrode,  a 
millivolt  less  than  the  value  (0.337  volt)  which  most  biological  investi- 
gators have  assigned  to  this  electrode.  However,  if  the  latter  value  is 
adopted  the  table  can  still  be  used ;  it  is  merely  necessary  to  shift  the 
values  given  under  the  column  EN  one  millivolt.  For  the  dissociation 

10 

constant  of  water  we  have  taken 

Kw  =  1.012  X  10-14   (25°C) 
which  gives  a  concentration  of  H+  and  OH"  as 
VKw=  1.006  X  10-7. 

The  value  of  Kw  is  stated  by  Lewis,  Brighton,  and  Sebastian61  to  be 
correct  within  two  or  three  per  cent.  All  calculations  in  the  table 
have  been  made  on  the  temperature  basis  of  25° C.  This  value  has 
been  most  generally  used  for  physico-chemical  work  and  is  well  within 
the  range  of  room  temperature  in  laboratories  having  no  special  facili- 
ties for  temperature  regulation.  For  small  temperature  variations 
this  error,  as  will  be  shown  later,  is  usually  negligible. 

For  the  calcuation  of  hydrogen  ion  concentration  (CH)  the  well- 
known  Nernst  equation 

RT  ,      1        * 
In 


nF    "(CH) 
is  used,  where 

E,  r=:gas  constant  in  volt  coulombs  (8.31574). 

T  =  absolute  temperature  (273.09  +  25). 

n  =  valency  of  hydrogen  (1). 

F  =  Faraday  constant  (96,500  coulombs). 

In  =  natural  logarithm.     In    -—  =  log  M 


TT    =  difference  of  potential  between  the  E.M.F.  measured  and 

the  potential  of  the  particular  calomel  cell  used. 
CH  =  concentration  of  hydrogen  ion  to  be  determined. 

At  25  °C  we  have 

,r  =  0.059152  Iog10  -^  =  0.059152  PH. 
_  CH 

*  To  be  more  exact,  according  to  recent  physico-chemical  views  it  is  the  activity 
of  the  H-ion  rather  than  the  concentration  which  is  measured.  Numerically, 
however,  the  value  is  the  same. 


26  University  of  California  Publications  in  Physiology      [VOL.  5 

This  equation  gives  at  once  both  the  values  for  PH  and  CH-    To  illus- 
trate :  when  the  voltage,  using  the  N/10  KCl-calomel  electrode,  is  0.773 

0.773  —  0.336  =  0.059152  PH  —  0.059152  Iog10  ^~ 
PH  =  7.388 


H  =  Iog10 


CH 
1 


CH  =  antilog. 

JL  H 

CH  =  10.000  — 10 
-7.388 

2.612  —  10  or —7  X  1.612 
CH  =  0.409  X  10-7 

1.012  X  IP"4      _o47vlo-T 
0.409  X10-7 

The  values  calculated  for  CH  and  PH  have  been  carried  to  three 
decimals  and  those  for  COH  to  two  decimals.  These  are  accurate  to 
one  unit  in  the  last  decimal  place.  For  most  purposes,  however,  it  is 
sufficiently  accurate  to  express  values  one  decimal  place  less  than  given 
in  the  table. 

The  results  given  in  the  tables  are  based  on  a  hydrogen  pressure 
of  760  millimeters.  It  requires  a  considerable  divergence  from  this 
pressure  to  produce  a  change  in  voltage  within  the  accuracy  of  the 
tables.  Loomis  and  Acree65  have  investigated  the  influence  of  pressure 
on  the  hydrogen  electrode  and  found  that  a  change  of  forty  milli- 
meters in  the  barometric  pressure  produced  a  change  in  the  potential 
of  only  0.0007  volt.  It  is  evident  that  the  ordinary  barometric  fluctua- 
tions are  of  no  significance  except  in  physico-chemical  researches.  If 
necessary,  however,  to  correct  for  partial  hydrogen  pressures,  it  may 
be  done  as  follows: 

Eb    =  E.M.F.  measured  at  the  barometric  pressure  b. 
eb      =  Eb  —  0.336  (for  the  N/  KCl-calomel  electrode) . 

0.05915    .        760 
e760  =  eb  ±  -    — log  ~^- 

E760  =  e760  +  0.336. 

The  correction  will  be  positive  when  b  is  less,  and  negative  when 
greater  than  760  millimeters. 

Temperature  has  a  somewhat  greater  influence  on  the  potential 
of  the  hydrogen  electrode,  and  varies  with  the  range  of  CH+  measured. 
Since  our  tables  have  been  calculated  on  the  temperature  basis  of 


1919]       Schmidt-Hoagland:  Table  of  PH,  H+  and  OH-  Values          27 

25 °C,  it  will  be  necessary,  if  measurements  are  made  at  any  other 
temperature,  to  convert  the  measured  voltage  to  the  value  it  would 
have  at  25 °C.  Within  ordinary  temperature  ranges  the  value  for  the 
calomel  cell  on  the  basis  of  PH  —  0  will  not  change,  hence  it  is  merely 
necessary  to  correct  et. 

Et  =  voltage  measured  at  the  temperature  t. 

et    =Et  —  0.336  (when  the  N/10  KCl-calomel  electrode 

is  used). 

e25   =  et  X  Factor. 
E,5  =  voltage  at  25° C. 
E25  =  e25  + 0.336. 

•pm 

From  the  Nernst  equation  it  will  be  seen  that  the  value  for—  —will 

nF 

change  with  the  temperature,  since  T  is  the  variable.  "We  have  calcu- 
lated a  series  of  factors  for  use  within  ordinary  temperature  ranges 
for  the  conversion  of  et  to  the  value  e25. 

Temperature  Factor  (Multiply) 

18  1.024 

19  1.021 

20  1.017 

21  1.014 

22  1.010 

23  1.007 

24  1.004 

25  1.000 

26  0.996 

27  0.993 

28  0.990 

29  0.987 

30  0.983 

At  the  neutral  point  the  change  in  voltage  per  degree  of  temperature 
variation  will  be  about  two  millivolts,  for  PH  =  4  this  will  be  only 
one  millivolt,  and  for  PH  =  11  it  will  rise  to  about  three  millivolts. 

The  large  variety  of  apparatus  used  by  different  authors  gives  the 
investigator  considerable  choice  for  the  particular  purpose  intended. 
For  many  biological,  bacteriological,  and  agricultural  investigations 
measurements  accurate  to  two  millivolts  are  within  the  limits  of 
interpretation.  For  this  purpose  the  method  outlined  by  Hildebrand27 
and  used  extensively  by  Sharp  and  Hoagland,365'  37°  in  which  the 
voltage  is  directly  measured  by  a  voltmeter,  is  well  adapted.  The 
direct-reading  potentiometer  of  Bovie2  is  useful  for  certain  types  of 
work.  Where  greater  accuracy  is  required,  such  as  the  standardiza- 


28  University  of  California  Publications  in  Physiology      [VOL.  5 

tion  of  buffer  mixtures,  reaction  changes  occurring  in  the  digestion 
of  proteins  by  enzymes  and  the  dissociation  of  proteins,  the  use  of 
a  potentiometer  with  a  sensitive  galvanometer  is  essential.  The 
potentiometer  manufactured  by  Leeds  and  Northrup  is  very  con- 
venient for  this  purpose. 

Rapidity  combined  with  accuracy  is  obtained  by  shaking  the 
solution  in  contact  with  the  hydrogen  gas  and  electrode.  For  many 
purposes  equilibrium  may  be  quickly  obtained  by  shaking  the  vessel 
by  hand;  more  convenient,  however,  are  the  motor-driven  shakers. 
For  this  purpose  the  electrode  vessel  designed  by  Clark3  and  used 
extensively  by  Clark  and  Lubs111  is  most  convenient.  Hydrogen  is 
best  generated  electrolytically.  Electrolysis  of  a  25  per  cent  KOH 
solution  using  nickel  electrodes,  or  a  6  per  cent  H2S04  solution  using 
platinum  electrodes  and  elimination  of  oxygen  or  ozone  by  passing 
the  hydrogen  over  heated  platinized  asbestos,  gives  a  very  pure 
product.  Compressed  hydrogen  from  cylinders  adequately  purified 
may  also  be  used.  We  have  always  used  the  Cottrell  gauze  electrode118 
since  it  is  easily  made  and  gives  a  large  surface.  Others  have  pre- 
ferred an  electrode  made  of  a  small  sheet  of  platinum.  This  is  coated 
with  platinum  black  by  deposition  in  a  solution  of  H2PtCl6  containing 
a  trace  of  lead  acetate.  Lewis,  Brighton,  and  Sebastian01  prefer  an 
electrode  of  gold  coated  with  iridium.  For  biological  work  it  is 
essential  that  the  electrode  be  saturated  with  hydrogen  before  immers- 
ing in  the  solution  to  be  tested. 

The  best  methods  of  evaluating  the  contact  potential  occurring  at 
the  junction  of  two  liquids  would  be  either  by  direct  determination 
or  by  calculation,  but  since  for  most  work  neither  of  these  methods 
can  at  present  be  used,  it  is  necessary  to  reduce  the  contact  potential 
to  a  minimum  by  interposing  a  saturated  solution  of  KC1  between  the 
solution  to  be  tested  and  the  calomel  electrode.  For  this  purpose  we 
use  glass  U  tubes  filled  by  placing  in  a  heated  solution  of  2  per  cent 
washed  agar  saturated  with  KCL  On  cooling  the  agar  solidifies  and 
the  KC1  in  part  crystallizes.  A  fresh  boundary,  obtained  by  cutting 
small  portions  off  the  ends  of  the  glass  tube,  should  be  used  for  each 
determination.  Sand  tubes,  string  dipped  in  a  saturated  KC1  solution 
or  a  beaker  containing  the  saturated  KC1  solution,  into  which  an 
arm  of  the  electrode  vessel  dips,  diffusion  being  prevented  by  using 
ungreased  stopcocks,  have  also  been  used.  In  measuring  such  systems 
as  soil  suspensions,  certain  protein  solutions,  etc.,  contamination  from 
the  KC1  should  be  avoided  by  the  use  of  a  side  arm  or  by  leaving 


1919]       Schmidt-Hoagland:  Table  of  PH,  H+  and  OH-  Values  29 

the  agar  tube  in  contact  with  the  solution  for  a  minimum  time,  other- 
wise interreactions  may  produce  changes  in  the  H+  concentration. 
For  most  work  the  magnitude  of  the  contact  potential  when  a  satu- 
rated solution  of  KC1  is  interposed  is  so  small  that  it  can  be  neglected. 
For  very  accurate  work  the  extrapolation  method  of  Bjerrum88  gives 
the  closest  approximation. 

Potential  measurements  of  systems  in  which  C02  is  a  determining 
factor  in  the  reaction  should  be  carried  out  in  closed  vessels,  equi- 
librium being  obtained  by  shaking.  The  methods  used  for  determining 
the  reaction  of  blood  and  body  fluids  are  well  adapted  for  this  pur- 
pose. In  soil  extracts  and  nutrient  solutions  for  plants  an  increase 
of  alkalinity  may  result  from  the  catalytic  reduction  of  the  N03  ion 
by  the  hydrogen  gas.  In  solutions  of  high  buffer  value  this  effect 
does  not  result  in  any  appreciable  change  in  H-ion  concentration,  but 
in  some  solutions  a  serious  error  may  be  caused.  It  has  been  noted 
that  thick  coatings  of  platinum  black  have  a  much  greater  catalytic 
power  than  thin  coatings ;  suitable  precautions  should  be  taken  there- 
fore when  measuring  solutions  containing  nitrates.  A  reduction  of 
nitrates  will  be  apparent  in  the  gradual  increase  of  voltage  during  the 
determination.  Under  these  circumstances  a  constant  value  cannot 
be  obtained. 

There  is  very  little  choice  between  the  normal  and  the  N/10  KC1- 
calomel  electrodes,  since  both  are  easily  reproducible  and  remain 
constant.  The  saturated  KCl-calomel  electrode  is  less  constant  and 
has  a  greater  temperature  variation  than  either  of  the  other  calomel 
electrodes.  Pure  materials  are  necessary.  For  this  purpose  the 
methods  described  by  Loomis  and  Acree63  and  Hildebrand103  are  well 
adapted.  The  glass  vessels  for  the  calomel  electrode  are  designed  to 
prevent  contamination  of  the  electrode  solution  and  to  provide  a 
method  for  washing  out  the  side  arm  with  KC1  solution.  A  convenient 
apparatus  is  described  by  Schmidt.272 

For  many  purposes  the  use  of  indicators  is  a  convenience.  Many 
of  the  indicators  used  by  Friedenthal,398  Salm,415  and  others  have 
largely  been  supplanted  by  indicators  of  the  sulfonphthalein 
series,404' 405  which  offer  more  convenient  ranges  of  color  change. 
These  have  been  extensively  described  by  Clark  and  Lubs.337  For 
some  work  it  is  necessary  to  test  the  applicability  of  a  particular 
indicator  by  determination  of  the  reaction  by  the  electrometric  method. 

The  use  of  buffer  mixtures  for  the  production  of  solutions  contain- 
ing definite  concentrations  of  hydrogen  ions  has  found  extensive 


30  University  of  California  Publications  in  Physiology      [VOL.  5 

application.  A  good  method  whereby  the  accuracy  of  a  hydrogen 
electrode  system  may  be  tested  consists  in  the  determination  of  the 
acidity  or  alkalinity  of  a  carefully  prepared  buffer  mixture.  The 
range  of  an  indicator  may  likewise  be  tested  this  way.  Buffer  mixtures 
are  usually  solutions  of  acetates,  bicarbonates,  borates,  phosphates, 
phthalates,  or  cacodylates.  These  have  been  carefully  standardized 
and  described  in  the  work  of  Sorensen,38  Palitzsch,113  Clark111  and 
others. 


Schmidt-Hoagland:  Table  of  PH?  H+  <md  OH-  Values     31 


TABLES 

EN 

EN- 

PH 

CH+ 

COH- 

1 

ID 

X  NH+ 

X  10-14  OH- 

0.283 

0.336 

1.000 

1.01 

0.285 

0.338 

0.034 

0.925 

1.09 

0.287 

0.340 

0.068 

0.856 

1.18 

0.289 

0.342 

0.101 

0.792 

1.28 

0.291 

0.344 

0.135 

0.732 

1.38 

0.293 

0.346 

0.169 

0.678 

1.49 

0.295 

0.348 

0.203 

0.627 

1.61 

0.297 

0.350 

0.237 

0.580 

1.75 

0.299 

0.352 

0.270 

0.536 

1.89 

0.301 

0.354 

0.304 

0.496 

2.04 

0.303 

0.356 

0.338 

0.459 

2.20 

0.305 

0.358 

0.372 

0.425 

2.38 

0.307 

0.360 

0.406 

0.393 

2.58 

0.309 

0.362 

0.440 

0.364 

2.78 

0.311 

0.364 

0.473 

0.336 

3.01 

0.313 

0.366 

0.507 

0.311 

3.25 

0.315 

0.368 

0.541 

0.288 

3.51 

0.317 

0.370 

0.575 

0.266 

3.80 

0.319 

0.372 

0.609 

0.246 

4.11 

0.321 

0.374 

0.642 

0.228 

4.44 

0.323 

0.376 

0.676 

0.211 

4.80 

0.325 

0.378 

0.710 

0.195 

5.19 

0.327 

0.380 

0.744 

0.180 

5.62 

0.329 

0.382 

0.778 

0.167 

6.06 

0.331 

0.384 

0.811 

0.154 

6.57 

0.333 

0.386 

0.845 

0.143 

7.08 

0.335 

0.388 

0.879 

0.132 

7.67 

0.337 

0.390 

0.913 

0.122 

8.30 

0.339 

0.392 

0.947 

0.113 

8.96 

0.341 

0.394 

0.980 

0.105 

9.64 

EN 

EN 

PH 

CH+ 

COH- 

~i 

10 

X  10-1  E> 

X  10-13  OH- 

0.343 

0.396 

1.014 

0.968 

1.05 

0.345 

0.398 

1.048 

0.895 

1.13 

0.347 

0.400 

1.082 

0.828 

1.22 

0.349 

0.402 

1.116 

0.766 

1.32 

0.351 

0.404 

1.150 

0.709 

1.43 

0.353 

0.406 

1.183 

0.656 

1,54 

0.355 

0.408 

1.217 

0.607 

1.67 

0.357 

0.410 

1.251 

0.561 

1.80 

0.359 

0.412 

1.285 

0.519 

1.95 

0.361 

0.414 

1.319 

0.480 

2.11 

0.363 

0.416 

1.352 

0.444 

2.28 

0.365 

0.418 

1.386 

0.411 

2.46 

0.367 

0.420 

1.420 

0.380 

2.66 

32     University  of  California  Publications  in  Physiology     [VOL.  5 


Ex 

EN 

PH 

CH+ 

COH- 

1 

Io 

X  10-1  H> 

X  10-13  OH- 

0.369 

0.422 

1.454 

0.352 

2.88 

0.371 

0.424 

1.488 

0.325 

3.11 

0.373 

0.426 

1.521 

0.301 

3.36 

0.375 

0.428 

1.555 

0.278 

3.64 

0.377 

0.430 

1.589 

0.258 

3.92 

0.379 

0.432 

1.623 

0.238 

4.25 

0.381 

0.434 

1.657 

0.221 

4.58 

0.383 

0.436 

1.691 

0.204 

4.96 

0.385 

0.438 

1.724 

0.189 

5.35 

0.387 

0.440 

1.758 

0.175 

5.78 

0.389 

0.442 

1.792 

0.162 

6.25 

0.391 

0.444 

1.826 

0.149 

6.79 

0.393 

0.446 

1.860 

0.138 

7.33 

0.395 

0.448 

1.893 

0.128 

7.91 

0.397 

0.450 

1.927 

0.118 

8.58 

0.399 

0.452 

1.961 

0.109 

9.28 

0.401 

0.454 

1.995 

0.101 

10.00 

EN 

EN 

PH 

CH+ 

COH- 

i 

10 

X  10-2  H+ 

X  10-12  OH- 

0.403 

0.456 

2.029 

0.936 

1.08 

0.405 

0.458 

2.062 

0.866 

1.17 

0.407 

0.460 

2.096 

0.801 

1.26 

0.409 

0.462 

2.130 

0.741 

1.37 

0.411 

0.464 

2.164 

0.686 

1.48 

0.413 

0.466 

2.198 

0.634 

1.60 

0.415 

0.468 

2.232 

0.587 

1.72 

0.417 

0.470 

2.265 

0.543 

1.86 

0.419 

0.472 

2.299 

0.502 

2.02 

0.421 

0.474 

2.333 

0.465 

2.18 

0.423 

0.476 

2.367 

0.430 

2.35 

0.425 

0.478 

2.401 

0.398 

2.54 

0.427 

0.480 

2.434 

0.368 

2.75 

0.429 

0.482 

2.468 

0.340 

2.98 

0.431 

0.484 

2.502 

0.315 

3.21 

0.433 

0.486 

2.536 

0.291 

3.48 

0.435 

0.488 

2.570 

0.269 

3.76 

0.437 

0.490 

2.603 

0.249 

4.06 

0.439 

0.492 

2.637 

0.231 

4.38 

0.441 

0.494 

2.671 

0.213 

4.75 

0.443 

0.496 

2.705 

0.197 

5.14 

0.445 

0.498 

2.739 

0.183 

5.53 

0.447 

0.500 

2.772 

0.169 

5.99 

0.449 

0.502 

2.806 

0.156 

6.49 

0.451 

0.504 

2.840 

0.145 

6.98 

0.453 

0.506 

2.874 

0.134 

7.55 

0.455 

0.508 

2.908 

0.124 

8.16- 

0.457 

0.510 

2.942 

0.114 

8.88 

0.459 

0.512 

2.975 

0.106 

9.55 

Schmidt-Hoagland:  Table  of  PH,  H+  and  OH-  Values     33 


EN 

EN 

PH 

CH+ 

COH- 

1 

To 

X  10-"  B> 

X  10-11  OH- 

0.461 

0.514 

3.009 

0.979 

1.03 

0.463 

0.516 

3.043 

0.906 

1.12 

0.465 

0.518 

3.077 

0.838 

1.21 

0.467 

0.520 

3.111 

0.775 

1.31 

0.469 

0.522 

3.144 

0.717 

1.41 

0.471 

0.524 

3.178 

0.663 

1.53 

0.473 

0.526 

3.212 

0.614 

1.65 

0.475 

0.528 

3.246 

0.568 

1.78 

0.477 

0.530 

3.280 

0.525 

1.93 

0.479 

0.532 

3.313 

0.486 

2.08 

0.481 

0.534 

3.347 

0.450 

2.25 

0.483 

0.536 

3.381 

0.416 

2.43 

0.485 

0.538 

3.415 

0.385 

2.63 

0.487 

0.540 

3.449 

0.356 

2.84 

0.489 

0.542 

3.483 

0.329 

3.08 

0.491 

0.544 

3.516 

0.305 

3.32 

0.493 

0.546 

3.550 

0.282 

3.59 

0.495 

0.548 

3.584 

0.261 

3.88 

0.497 

0.550 

3.618 

0.241 

4.20 

0.499 

0.552 

3.652 

0.223 

4.54 

0.501 

0.554 

3.685 

0.206 

4.91 

0.503 

0.556 

3.719 

0.191 

5.30 

0.505 

0.558 

3.753 

0.177 

5.72 

0.507 

0.560 

3.787 

0.163 

6.21 

0.509 

0.562 

3.821 

0.151 

6.70 

0.511 

0.564 

3.854 

0.140 

7.23 

0.513 

0.566 

3.888 

0.129 

7.85 

0.515 

0.568 

3.922 

0.120 

8.43 

0.517 

0.570 

3.956 

0.111 

9.12 

0.519 

0.572 

3.990 

0.102 

9.92 

EN 

EN 

PH 

CH+ 

COH- 

~T 

To 

X  10-4  B> 

X  10-10  OH 

0.521 

0.574 

4.023 

0.947 

1.07 

0.522 

0.575 

4.040 

0.911 

1.11 

0.523 

0.576 

4.057 

0.876 

1.16 

0.524 

0.577 

4.074 

0.843 

1.20 

0.525 

0.578 

4.091 

0.811 

1.25 

0.526 

0.579 

4.108 

0.780 

1.30 

0.527 

0.580 

4.125 

0.750 

1.35 

0.528 

0.581 

4.142 

0.721 

1.40 

0.529 

0.582 

4.159 

0.694 

1.46 

0.530 

0.583 

4.176 

0.667 

1.52 

0.531 

0.584 

4.193 

0.642 

1.58 

0.532 

0.585 

4.210 

0.617 

1.64 

0.533 

0.586 

4.226 

0.594 

1.70 

0.534 

0.587 

4.243 

0.571 

1.77 

0.535 

0.588 

4.260 

0.549 

1.84 

0.536 

0.589 

4.277 

0.528 

1.92 

0.537 

0.590 

4.294 

0.508 

1.99 

0.538 

0.591 

4.311 

0.489 

2.07 

34     University  of  California  Publications  in  Physiology     [VOL.  5 


EN 

EN 

PH 

CH+ 

COH- 

1 

10 

X  10-"  H> 

X  10-10  OH- 

0.539 

0.592 

4.328 

0.470 

2.15 

0.540 

0.593 

4.345 

0.452 

2.24 

0.541 

0.594 

4.362 

0.435 

2.33 

0.542 

0.595 

4.379 

0.418 

2.42 

0.543 

0.596 

4.395 

0.402 

2.52 

0.544 

0.597 

4.412 

0.387 

2.61 

0.545 

0.598 

4.429 

0.372 

2.72 

0.546 

0.599 

4.446 

0.358 

2.83 

0.547 

0.600 

4.463 

0.344 

2.94 

0.548 

0.601 

4.480 

0.331 

3.06 

0.549 

0.602 

4.497 

0.319 

3.17 

0.550 

0.603 

4.514 

0.306 

3.31 

0.551 

0.604 

4.531 

0.295 

3.43 

0.552 

0.605 

4.548 

0.283 

3.58 

0.553 

0.606 

4.564 

.  0.273 

3.71 

0.554 

0.607 

4.581 

0.262 

3.86 

0.555 

0.608 

4.598 

0.252 

4.02 

0.556 

0.609 

4.'615 

0.243 

4.16 

0.557 

0.610 

4.632 

0.233 

4.34 

0.558 

0.611 

4.649 

0.224 

4.52 

0.559 

0.612 

4.666 

0.216 

4.69 

0.560 

0.613 

4.683 

0.208 

4.87 

0.561 

0.614 

4.700 

0.200 

5.06 

0.562 

0.615 

4.717 

0.192 

5.27 

0.563 

0.616 

4.734 

0.185 

5.47 

0.564 

0.617 

4.750 

0.178 

5.69 

0.565 

0.618 

4.767 

0.171 

5.92 

0.566 

0.619 

4.784 

0.164 

6.17 

0.567 

0.620 

4.801 

0.158 

6.41 

0.568 

0.621 

4.818 

0.152 

6.66 

0.569 

0.622 

4.835 

0.146 

6.93 

0.570 

0.623 

4.852 

0.141 

7.18 

0.571 

0.624 

4.869 

0.135 

7.50 

0.572 

0.625 

4.886 

0.130 

7.78 

0.573 

0.626 

4.903 

0.125 

8.10 

0.574 

0.627 

4.920 

0.120 

8.43 

0.575 

0.628 

4.936 

0.116 

8.72 

0.576 

0.629 

4.953 

0.111 

9.12 

0.577 

0.630 

4.970 

0.107 

9.46 

0.578 

0.631 

4.987 

0.103 

9.83 

EN 

EN 

PH 

CH+ 

COH- 

1 

To 

X  10-5  H+ 

X  10-9  OH- 

0.579 

0.632 

5.004 

o'.991 

1.02 

0.580 

0.633 

5.021 

0.953 

1.06 

0.581 

0.634 

5.038 

0.916 

1.10 

0.582 

0.635 

5.055 

0.881 

1.15 

0.583 

0.636 

5.072 

0.848 

1.19 

0.584 

0.637 

5.089 

0.815 

1.24 

0.585 

0.638 

5.106 

0.784 

1.29 

0.586 

0.639 

5.122 

0.754 

1.34 

Schmidt-Hoagland:  Table  of  PH,  H+  wnd  OH-  Values     35 


EN 

Ex 

PH 

CH+ 

COH- 

i 

To 

X  10-5  H> 

X  10-"  OH- 

0.587 

0.640 

5.139 

0.725 

1.40 

0.588 

0.641 

5.156 

0.698 

1.45 

0.589 

0.642 

5.173 

0.671 

1.51 

0.590 

0.643 

5.190 

0.646 

1.57 

0.591 

0.644 

5.207 

0.621 

1.63 

0.592 

0.645 

5.224 

0.597 

1.70 

0.593 

0.646 

5.241 

0.574 

1.76 

0.594 

0.647 

5.258 

0.552 

1.83 

0.595 

0.648 

5.275 

0.531 

1.91 

0.596 

0.649 

5.292 

0.511 

1.98 

0.597 

0.650 

5.308 

0.492 

2.06 

0.598 

0.651 

5.325 

0.473 

2.14 

0.599 

0.652 

5.342 

0.455 

2.22 

0.600 

0.653 

5.359 

0.437 

2.32 

0.601 

0.654 

5.376 

0.421 

2.40 

0.602 

0.655 

5.393 

0.405 

2.50 

0.603 

0.656 

5.410 

0.390 

2.59 

0.604' 

0.657 

5.427 

0.374 

2.71 

0.605 

0.658 

5.444 

0.360 

2.81 

0.606 

0.659 

5.461 

0.346 

2.92 

0.607 

0.660 

5.478 

0.333 

3.04 

0.608 

0.661 

5.495 

0.320 

3.16 

0.609 

0.662 

5.511 

0.308 

3.29 

0.610 

0.663 

5.528 

0.296 

3.42 

0.611 

0.664 

5.545 

0.285 

3.55 

0.612 

0.665 

5.562 

0.274 

3.69 

0.613 

0.666 

5.579 

0.264 

3.83 

0.614 

0.667 

5.596 

0.254 

3.98 

0.615 

0.668 

5.613 

0.244 

4.15 

0.616 

0.669 

5.630 

0.235 

4.31 

0.617 

0.670 

5.647 

0.226 

4.48 

0.618 

0.671 

5.664 

0.217 

4.66 

0.619 

0.672 

5.681 

0.209 

4.84 

0.620 

0.673 

5.697 

0.201 

5.03 

0.621 

0.674 

5.714 

0.193 

5.24 

0.622 

0.675 

5.731 

0.186 

5.44 

0.623 

0.676 

5.748 

0.179 

5.65 

0.624 

0.677 

5.765 

0.172 

5.88 

0.625 

0.678 

5.782 

0.165 

6.13 

0.626 

0.679 

5.799 

0.159 

6.36 

0.627 

0.680 

5.816 

0.153 

6.61 

0.628 

0.681 

5.833 

0.147 

6.88 

0.629 

0.682 

5.850 

0.141 

7.18 

0.630 

0.683 

5.866 

0.136 

7.44 

0.631 

0.684 

5.883 

0.131 

7.73 

0.632 

0.685 

5.900 

0.126 

8.03 

0.633 

0.686 

5.917 

0.121 

8.36 

0.634 

0.687 

5.934 

0.116 

8.72 

0.635 

0.688 

5.951 

0.112 

9.04 

0.636 

0.689 

5.968 

0.108 

9.37 

0.637 

0.690 

5.985 

0.104 

9.73 

36     University  of  California  Publications  in  Physiology     [VOL.  5 


EN 

EN 

PH 

CH+ 

COH- 

T 

10 

X  10-6  B> 

X  10-8  OH 

0.638 

0.691 

6.002 

0.996 

1.02 

0.639 

0.692 

6.019 

0.958 

1.06 

0.640 

0.693 

6.036 

0.921 

1.10 

0.641 

0.694 

6.052 

0.886 

1.14 

0.642 

0.695 

6.069 

0.852 

1.19 

Oi643 

0.696 

6.086 

0.820 

1.23 

0.644 

0.697 

6.103 

0.789 

1.28 

0.645 

0.698 

6.120 

0.758 

1.34 

0.646 

0.699 

6.137 

0.729 

1.39 

0.647 

0.700 

6.154 

0.702 

1.44 

0.648 

0.701 

6.171 

0.675 

1.50 

0.649 

0.702 

6.188 

0.649 

1.56 

0.650 

0.703 

6.204 

0.625 

1.62 

0.651 

0.704 

6.221 

0.601 

1.68 

0.652 

0.705 

6.238 

0.578 

1.75 

0.653 

0.706 

6.255 

0.556 

1.82 

0.654 

0.707 

6.272 

0.535 

1.89 

0.655 

0.708 

6.289 

0.514 

1.97 

0.656 

0.709 

6.306 

0.495 

2.04 

0.657 

0.710 

6.323 

0.476 

2.13 

0.658 

0.711 

6.340 

0.458 

2.21 

0.659 

0.712 

6.357 

0.440 

2.30 

0.660 

0.713 

6.373 

0.423 

2.39 

0.661 

0.714 

6.390 

0.407 

2.49 

0.662 

0.715 

6.407 

0.392 

2.58 

0.663 

0.716 

6.424 

0.377 

2.68 

0.664 

0.717 

6.441 

0.362 

2.80 

0.665 

0.718 

6.458 

0.348 

2.91 

0.666 

0.719 

6.475 

0.335 

3.02 

0.667 

0.720 

6.492 

0.322 

3.14 

0.668 

0.721 

6.509 

0.310 

3.26 

0.669 

0.722 

6.526 

0.298 

3.40 

0.670 

0.723 

6.543 

0.287 

3.53 

0.671 

0.724 

6.559 

0.276 

3.67 

0.672 

.  0.725 

6.576 

0.265 

3.82 

0.673 

0.726 

6.593 

0.255 

3.97 

0.674 

0.727 

6.610 

0.245 

4.13 

0.675 

0.728 

6.627 

0.236 

4.29 

0.676 

0.729 

6.644 

0.227 

4.46 

0.677 

0.730 

6.661 

0.218 

4.64 

0.678 

0.731 

6.678 

0.210 

4.82 

0.679 

0.732 

6.695 

0.202 

5.01 

0.680 

0.733 

6.712 

0.194 

5.22 

0.681 

0.734 

6.728 

0.187 

5.41 

0.682 

0.735 

6.745 

0.180 

5.62 

0.683 

0.736 

6.762 

0.173 

5.85 

0.684 

0.737 

6.779 

0.166 

6.10 

0.685 

0.738 

6.796 

0.160 

6.32 

0.686 

0.739 

6.813 

0.154 

6.57 

0.687 

0.740 

6.830 

0.148 

6.84 

Schmidt-Hoagland:  Table  of  PH,  H+  and  OR-  Values     37 


EN 

EN 

PH 

CH+ 

COH- 

~1 

10 

X  10-8  H+ 

X  10-8  OH 

0.688 

0.741 

6.847 

0.142 

7.13 

0.689 

0.742 

6.864 

0.137 

7.39     ' 

0.690 

0.743 

6.881 

0.132 

7.67 

0.691 

0.744 

6.898 

0.127 

7.97 

0.692 

0.745 

6.914 

0.122 

8.30 

0.693 

0.746 

6.931 

0.117 

8.65 

0.694 

0.747 

6.948 

0.113 

8.96 

0.695 

0.748 

6.965 

0.108 

9.37 

0.696 

0.749 

6.982 

0.104 

9.73 

*0.697 

0.750 

6.999 

0.100 

10.12 

EN 

EN 

PH 

CH+ 

COH- 

1 

10 

X  10-7  H+ 

X  10-T  OH 

0.698 

0.751 

7.016 

0.964 

1.05 

0.699 

0.752 

7.033 

0.927 

1.09 

0.700 

0.753 

7.050 

0.892 

1.13 

0.701 

0.754 

7.067 

0.858 

1.18 

0.702 

0.755 

7.084 

0.825 

1.23 

0.703 

0.756 

7.100 

0.794 

1.27 

0.704 

0.757 

7.117 

0.763 

1.33 

0.705 

0.758 

7.134 

0.734 

1.38 

0.706 

0.759 

7.151 

0.706 

1.43 

0.707 

0.760 

7.168 

0.679 

1.49 

0.708 

0.761 

7.185 

0.653 

1.55 

0.709 

0.762 

7.202 

0.628 

1.61 

0.710 

0.763 

7.219 

0.604 

1.68 

0.711 

0.764 

7.236 

0.581 

1.74 

0.712 

0.765 

7.253 

0.559 

1.81 

0.713 

0.766 

7.269 

0.538 

1.88 

0.714 

0.767 

7.286 

0.517 

1.96 

0.715 

0.768 

7.303 

0.497 

2.04 

0.716 

0.769 

7.320 

0.478 

2.12 

0.717 

0.770 

7.337 

0.460 

2.20 

0.718 

0.771 

7.354 

0.443 

2.28 

0.719 

0.772 

7.371 

0.426 

2.38 

0.720 

0.773 

7.388 

0.409 

2.47 

0.721 

0.774 

7.405 

0.394 

2.57 

0.722 

0.775 

7.422 

0.379 

2.67 

0.723 

0.776 

7.439 

0.364 

2.78 

0.724 

0.777 

7.455 

0.350 

2.89 

0.725 

0.778 

7.472 

0.337 

3.00 

0.726 

0.779 

7.489 

0.324 

3.12 

0.727 

0.780 

7.506 

0.312 

3.24 

0.728 

0.781 

7.523 

0.300 

3.37 

0.729 

0.782 

7.540 

0.288 

3.51 

0.730 

0.783 

7.557 

0.277 

3.65 

0.731 

0.784 

7.574 

0.267 

3.79 

0.732 

0.785 

7.591 

0.257 

3.94 

0.733 

0.786 

7.608 

0.247 

4.10 

*  Neutral  point. 


38     University  of  California  Publications  in  Physiology     [VOL.  5 


EN 

EN 

PH 

CH+ 

COH- 

1 

10 

X  10-7  B> 

X  10-7  OH 

0.734 

0.787 

7.624 

0.238 

4.25 

0.735 

0.788 

7.641 

0.228 

4.44 

0.736 

0.789 

7.658 

0.220 

4.60 

0.737 

0.790 

7.675 

0.211 

4.80 

0.738 

0.791 

7.692 

0.203 

4.99 

0.739 

0.792 

7.709 

0.195 

5.19 

0.740 

0.793 

7.726 

0.188 

5.38 

0.741 

0.794 

7.743 

0.181 

5.59 

0.742 

0.795 

7.760 

0.174 

5.82 

0.743 

0.796 

7.777 

0.167 

6.06 

0.744 

0.797 

7.794 

0.161 

6.29 

0.745 

0.798 

7.810 

0.155 

6.53 

0.746 

0.799 

7.827 

0.149 

6.79 

0.747 

0.800 

7.844 

0.143 

7.08 

0.748 

0.801 

7.861 

0.138 

7.33 

0.749 

0.802 

7.878 

0.132 

7.67 

0.750 

0.803 

7.895 

0.127 

7.97 

0.751 

0.804 

7.912 

0.123 

8.23 

0.752 

0.805 

7.929 

0.118 

8.58 

0.753 

0.806 

7.946 

0.113 

8.96 

0.754 

0.807 

7.963 

0.109 

9.28 

0.755 

0.808 

7.980 

0.105 

9.64 

0.756 

0.809 

7.996 

0.101 

10.02 

EN 

EN 

PH 

CH+ 

COH- 

i 

10 

X  10-8  H> 

X  10-"  OH 

0.757 

0.810 

8.013 

0.970 

1.04 

0.758 

0.811 

8.030 

0.933 

1.08 

0.759 

0.812 

8.047 

0.897 

1.13 

0.760 

0.813 

8.064 

0.863 

1.17 

0.761 

0.814 

8.081 

0.830 

1.22 

0.762 

0.815 

8.098 

0.798 

1.27 

0.763 

0.816 

8.115 

0.768 

1.32 

0.764 

0.817 

8.132 

0.739 

1.37 

0.765 

0.818 

8.149 

0.710 

1.43 

0.766 

0.819 

8.165 

0.683 

1.48 

0.767 

0.820 

8.182 

0.657 

1.54 

0.768 

0.821 

8.199 

0.632 

1.60 

0.769 

0.822 

8.216 

0.608 

1.66 

0.770 

0.823 

8.233 

0.585 

1.73 

0.771 

0.824 

8.250 

0.562 

1.80 

0.772 

0.825 

8.267 

0.541 

1.87 

0.773 

0.826 

8.284 

0.520 

1.95 

0.774 

0.827 

8.301 

0.500 

2.02 

0.775 

0.828 

8.318 

0.481 

2.10 

0.776 

0.829 

8.335 

0.463 

2.19 

0.777 

0.830 

8.351 

0.445 

2.27 

0.778 

0.831 

8.368 

0.428 

2.36 

0.779 

0.832 

8.385 

0.412 

2.46 

Schmidt-Hoagland:  Table  of  PH,  H+  and  OH-  Values     39 


EN 

EN 

PH 

CH+ 

COH- 

1 

10 

X  10-8  H> 

X  10-6  OH- 

0.780 

0.833 

8.402 

0.396 

2.56 

0.781 

0.834 

8.419 

0.381 

2.66 

0.782 

0.835 

8.436 

0.367 

2.76 

0.783 

0.836 

8.453 

0.353 

2.87 

0.784 

0.837 

8.470 

0.339 

2.99 

0.785 

0.838 

8.487 

0.326 

3.10 

0.786 

0.839 

8.504 

0.314 

3.22 

0.787 

0.840 

8.521 

0.302 

3.35 

0.788 

0.841 

8.537 

0.290 

3.49 

0.789 

0.842 

8.554 

0.279 

3.63 

0.790 

0.843 

8.571 

0.269 

3.76 

0.791 

0.844 

8.588 

0.258 

3.92 

0.792 

0.845 

8.605 

0.248 

4.08 

0.793 

0.846 

8.622 

0.239 

4.23 

0.794 

0.847 

8.639 

0.230 

4.40 

0.795 

0.848 

8.656 

0.221 

4.58 

0.796 

0.849 

8.673 

0.213 

4.75 

0.797 

0.850 

8.690 

0.204 

4.96 

0.798 

0.851 

8.706 

0.197 

5.14 

0.799 

0.852 

8.723 

0.189 

5.35 

0.800 

0.853 

8.740 

0.182 

5.56 

0.801 

0.854 

8.757 

0.175 

5.78 

0.802 

0.855 

8.774 

0.168 

6.02 

0.803 

0.856 

8.791 

0.162 

6.25 

0.804 

0.857 

8.808 

0.156 

6.49 

0.805 

0.858 

8.825 

0.150 

6.75 

0.806 

0.859 

8.842 

0.144 

7.03 

0.807 

0.860 

8.859 

0.139 

7.28 

0.808 

0.861 

8.876 

0.133 

7.61 

0.809 

0.862 

8.892 

0.128 

7.91 

0.810 

0.863 

8.909 

0.123 

8.23 

0.811 

0.864 

8.926 

0.119 

8.50 

0.812 

0.865 

8.943 

0.114 

8.88 

0.813 

0.866 

8.960 

0.110 

9.20 

0.814 

0.867 

8.977 

0.106 

9.55 

0.815 

0.868 

8.994 

0.101 

10.00 

EN 

EN 

PH 

CH+ 

COH- 

i 

To 

X  10-"  H+ 

X  10-B  OH 

0.816 

0.869 

9.011 

0.975 

1.04 

0.817 

0.870 

9.028 

0.938 

1.08 

0.818 

0.871 

9.045 

0.902 

1.12 

0.819 

0.872 

9.062 

0.868 

1.17 

0.820 

0.873 

9.078 

0.835 

1.21 

0.821 

0.874 

9.095 

0.803 

1.26 

0.822 

0.875 

9.112 

0.772 

1.31 

0.823 

0.876 

9.129 

0.743 

1.36 

0.824 

0.877 

9.146 

0.714 

1.42 

0.825 

0.878 

9.163 

0.687 

1.47 

40     University  of  California  Publications  m  Physiology     [VoL-  5 


EN 

EN 

PH 

CH+ 

COH- 

i 

10 

X  10-"  H> 

X  10-5  OH- 

0.826 

0.879 

9.180 

0.661 

1.53 

0.827 

0.880 

9.197 

0.636 

1.59 

0.828 

0.881 

9.214 

0.611 

1.66 

0.829 

0.882 

9.231 

0.588 

1.72 

0.830 

0.883 

9.248 

0.566 

1.79 

0.831 

0.884 

9.264 

0.544 

1.86 

0.832 

0.885 

9.281 

0.523 

1.93 

0.833 

0.886 

9.298 

0.503 

2.01 

0.834 

0.887 

9.315 

0.484 

2.09 

0.835 

0.888 

9.332 

0.466 

2.17 

0.836 

0.889 

9.349 

0.448 

2.26 

0.837 

0.890 

9.366 

0.431 

2.35 

0.838 

0.891 

9.383 

0.414 

2.44 

0.839 

0.892 

9.400 

0.398 

2.54 

0.840 

0.893 

9.417 

0.383 

2.64 

0.841 

0.894 

9.434 

0.369 

2.74 

0.842 

0.895 

9.450 

0.354 

2.86 

0.843 

0.896 

9.467 

0.341 

2.97 

0.844 

0.897 

9.484 

0.328 

3.09 

0.845 

0.898 

9.501 

0.315 

3.21 

0.846 

0.899 

9.518 

0.304 

3.33 

0.847 

0.900 

9.535 

0.292 

3.47 

0.848 

0.901 

9.552 

0.281 

3.60 

0.849 

0.902 

9.569 

0.270 

3.75 

0.850 

0.903 

9.585 

0.260 

3.89 

0.851 

0.904 

9.602 

0.250 

4.05 

0.852 

0.905 

9.619 

0.240 

4.22 

0.853 

0.906 

9.636 

0.231 

4.38 

0.854 

0.907 

9.653 

0.222 

4.56 

0.855 

0.908 

9.670 

0.214 

4.73 

0.856 

0.909 

9.687 

0.206 

4.91 

0.857 

0.910 

9.704 

0.198 

5.11 

0.858 

0.911 

9.721 

0.190 

5.33 

0.859 

0.912 

9.738 

0.183 

5.53 

0.860 

0.913 

9.755 

0.176 

5.75 

0.861 

0.914 

9.772 

0.169 

5.99 

0.862 

0.915 

9.788 

0.163 

6.21 

0.863 

0.916 

9.805 

0.157 

6.45 

0.364 

0.917 

9.822 

0.151 

6.70 

0.865 

0.918 

9.839 

0.145 

6.98 

0.866 

0.919 

9.856 

0.139 

7.28 

0.867 

0.920 

9.873 

0.134 

7.55 

0.868 

0.921 

9.890 

0.129 

7.84 

0.869 

0.922 

9.907 

0.124 

8.16 

0.870 

0.923 

9.924 

0.119 

8.50 

0.871 

0.924 

9.941 

0.115 

8.80 

0.872 

0.925 

9.958 

0.110 

9.20 

0.873 

0.926 

9.974 

0.106 

9.55 

0.874 

0.927 

9.991 

0.102 

9.92 

Schmidt-Hoagland:  Table  of  PH,  H+  and  OHr  Fate     41 


EN 

EN 

PH 

CH+ 

COH- 

1 

10 

X  10-10  H> 

X  10-4  OH- 

0.875 

0.928 

10.008 

0.981 

1.03 

0.877 

0.930 

10.042 

0.908 

1.11 

0.879 

0.932 

10.076 

0.840 

1.20 

0.881 

0.934 

10.110 

0.777 

1.30 

0.883 

0.936 

10.143 

0.719 

1.41 

0.885 

0.938 

10.177 

0.665 

1.52 

0.887 

0.940 

10.211 

0.615 

1.65 

0.889 

0.942 

10.245 

0.569 

1.78 

0.891 

0.944 

10.279 

0.526 

1.92 

0.893 

0.946 

10.313 

0.487 

2.08 

0.895 

0.948 

10.346 

0.451 

2.24 

0.897 

0.950 

10.380 

0.417 

2.43 

0.899 

0.952 

10.414 

0.386 

2.62 

0.901 

0.954 

10.448 

0.357 

2.83 

0.903 

0.956 

10.481 

0.330 

3.07 

0.905 

0.958 

10.515 

0.305 

3.32 

0.907 

0.960 

10.549 

0.282 

3.59 

0.909 

0.962 

10.583 

0.261 

3.88 

0.911 

0.964 

10.617 

0.242 

4.18 

0.913 

0.966 

10.651 

0.224 

4.52 

0.915 

0.968 

10.684 

0.207 

4.89 

0.917 

0.970 

10.718 

0.191 

5.30 

0.919 

0.972 

10.752 

0.177 

5.72 

0.921 

0.974 

10.786 

0.164 

6.17 

0.923 

0.976 

10.820 

0.152 

6.66 

0.925 

0.978 

10.853 

0.140 

7.23 

0.927 

0.980 

10.887 

0.130 

7.78 

0.929 

0.982 

10.921 

0.120 

8.43 

0.931 

0.984 

10.955 

0.111 

9.12 

0.933 

0.986 

10.989 

0.103 

9.83 

EN 

EN 

PH 

CH+ 

COH- 

i 

10 

X  10-11  H> 

X  10-3  OH- 

0.935 

0.988 

11.022 

0.950 

1.07 

0.937 

0.990 

11.056 

0.879 

1.15 

0.939 

0.992 

11.090 

0.813 

1.24 

0.941 

0.994 

11.124 

0.752 

1.35 

0.943 

0.996 

11.158 

0.696 

1.45 

0.945 

0.998 

11.191 

0.644 

1.57 

0.947 

1.000 

11.225 

0.595 

1.70 

0.949 

1.002 

11.259 

0.551 

1.84 

0.951 

1.004 

11.293 

0.509 

1.99 

0.953 

1.006 

11.327 

0.471 

2.15 

0.955 

1.008 

11.361 

0.436 

2.32 

0.957 

1.010 

11.394 

0.403 

2.51 

0.959 

1.012 

11.428 

0.373 

2.71 

0.961 

1.014 

11.462 

0.345 

2.93 

0.963 

1.016 

11.496 

0.319 

3.17 

0.965 

1.018 

11.530 

0.295 

3.43 

42     University  of  California  Publications  in  Physiology     [VOL.  5 


EN 

EN 

PH 

CH+ 

COH- 

i 

10 

X  10-11  H+ 

X  10-3  OH 

0.967 

1.020 

11.563 

0.273 

3.71 

0.969 

1.022 

11.597 

0.253 

4.00 

0.971 

1.024 

11.631 

0.234 

4.32 

0.973 

1.026 

11.665 

0.216 

4.69 

0.975 

1.028 

11.699 

0.200 

5.06 

0.977 

1.030 

11.732 

0.185 

5.47 

0.979 

1.032 

11.766 

0.171 

5.92 

0.981 

1.034 

11.800 

0.159 

6.36 

0.983 

1.036 

11.834 

0.147 

6.88 

0.985 

1.038 

11.868 

0.136 

7.44 

0.987 

1.040 

11.901 

0.126 

8.03 

0.989 

1.042 

11.935 

0.116 

8.72 

0.991 

1.044 

11.969 

0.107 

9.46 

EN 

EN 

PH 

CH+ 

COH- 

1 

10 

X  10-"  H+ 

X  10-2  OH- 

0.993 

1.046 

12.003 

0.993 

1.02 

0.995 

1.048 

12.037 

0.919 

1.10 

0.997 

1.050 

12.071 

0.850 

1.19 

0.999 

1.052 

12.104 

0.786 

1.29 

1.001 

1.054 

12.138 

0.728 

1.39 

1.003 

,1.056 

12.172 

0.673 

1.50 

1.005 

1.058 

12.206 

0.623 

1.62 

1.007 

1.060 

12.240 

0.576 

1.76 

1.009 

1.062 

12.273 

0.533 

1.90 

1.011 

1.064 

12.307 

0.493 

2.05 

1.013 

1.066 

12.341 

0.456 

2.22 

1.015 

1.068 

12.375 

0.422 

2.40 

1.017 

1.070 

12.409 

0.390 

2.59 

1.019 

1.072 

12.443 

0.361 

2.80 

1.021 

1.074 

12.476 

0.334 

3.03 

1.023 

1.076 

12.510 

0.309 

3.28 

1.025 

1.078 

12.544 

0.286 

3.54 

1.027 

1.080 

12.578 

0.264 

3.83 

1.029 

1.082 

12.612 

0.245 

4.13 

1.031 

1.084  ' 

12.645 

0.226 

4.48 

1.033 

1.086 

12.679 

0.209 

4.84 

1.035 

1.088 

12.713 

0.194 

5.22 

1.037 

1.090 

12.747 

0.179 

5.65 

1.039 

1.092 

12.781 

0.166 

6.10 

1.041 

1.094 

12.814 

0.153 

6.61 

1.043 

1.096 

12.848 

0.142 

7.13 

1.045 

1.098 

12.882 

0.131 

7.73 

1.047 

1.100 

12.916 

0.121 

8.36 

1.049 

1.102 

12.950 

0.112 

9.04 

1.051 

1.104 

12.983 

0.104 

9.73 

Schmidt-Hoagland:  Table  of  PH,  H+  and  OHr  Values     43 


EN 

EN 

PH 

CH+ 

COH- 

1 

10 

X  10~13  H+ 

X  10-1  OH 

1.053 

1.106 

13.017 

0.961 

1.05 

1.055 

1.108 

13.051 

0.889 

1.14 

1.057 

1.110 

13.085 

0.822 

1.23 

1.059 

1.112 

13.119 

0.761 

1.33 

1.061 

1.114 

13.153 

0.704 

1.44 

1.063 

1.116 

13.186 

0.651 

1.55 

1.065 

1.118 

13.220 

0.602 

1.68 

1.067 

1.120 

13.254 

0.557 

1.82 

1.069 

1.122 

13.288 

0.516 

1.96 

1.071 

1.124 

13.322 

0.477 

2.12 

1.073 

1.126 

13.355 

0.441 

2.29 

1.075 

1.128 

13.389 

0.408 

2.48 

1.077 

1.130 

13.423 

0.378 

2.68 

1.079 

1.132 

13.457 

0.349 

2.90 

1.081 

1.134 

13.491 

0.323 

3.13 

1.083 

1.136 

13.524 

0.299 

3.38 

1.085 

1.138 

13.558 

0.277 

3.65 

1.087 

1.140 

13.592 

0.256 

3.95 

1.089 

1.142 

13.626 

0.237 

4.27 

1.091 

1.144 

13.660 

0.219 

4.62 

1.093 

1.146 

13.693 

0.203 

4.99 

1.095 

1.148 

13.727 

0.187 

5.41 

1.097 

1.150 

13.761 

0.173 

5.85 

1.099 

1.152 

13.795 

0.160 

6.32 

1.101 

1.154 

13.829 

0.148 

6.84 

1.103 

1.156 

13.863 

0.137 

7.39- 

1.105 

1.158 

13.896 

0.127 

7.97 

1.107 

1.160 

13.930 

0.117 

8.65 

1.109 

1.162 

13.964 

0.109 

9.28 

1.111 

1.164 

13.998 

0.101 

10.02 

X  10-14  H+ 

X  NOH- 

1.113 

1.166 

14.032 

0.930 

1.09 

44     University  of  California  Publications  in  Physiology     [VOL.  5 


LITERATURE 

I.  GENERAL  AND  THEORETICAL. 

A.  APPAEATUS. 

1  Barendrecht,  H.  P.,  A  simple  hydrogen  electrode,  Biochem.  Jour., 
1915,  vol.  9,  pp.  66-70. 

2  Bovie,  W.  T.,  A  direct  reading  potentiometer  for  measuring  and 
recording  both  the  actual  and  the  total  reaction  of  solutions,  Jour. 
Med.  Ees.,  1915,  vol.  33,  pp.  295-322. 

s  Clark,-  W.  M.,  A  hydrogen  electrode  vessel,  Jour.  Biol.  Chem., 
1915,  vol.  23,  pp.  475-486. 

*  Liebermann,  L.  v.,  Platinelektroden  zur  Bestimmung  der  H- 
und  OH-  lonenkonzentration,  Chem.  Ztg.,  1911,  vol.  35,  p.  972. 

s  Long,  J.  H.,  A  simple  cell  for  the  determination  of  hydrogen 
ion  concentration,  Jour.  Am.  Chem.  Soc.,  1916,  vol.  38,  pp.  936-939. 

s  McClendon,  J.  F.,  New  hydrogen  electrodes  and  rapid  methods 
of  determining  hydrogen  ion  concentrations,  Am.  Jour.  Physiol.,  1915, 
vol.  38,  pp.  180-185. 

7  McClendon,  J.  F.,  A  direct  reading  potentiometer  for  measuring 
hydrogen  ion  concentrations,  Am.  Jour.  Physiol.,  1915,  vol.   38,   pp. 
186-190. 

8  McClendon,  J.  F.,  and  Magoon,  C.  A.,  An  improved  Hasselbalch 
hydrogen  electrode  and  a  combined  tonometer  and  hydrogen  electrode, 
together   with   rapid   methods   of    determining   the    buffer    value    of 
blood,  Jour.  Biol.  Chem.,  1916,  vol.  25,  pp.  669-681. 

9  Walpole,  G.  S.,  Gas-electrode  for  general  use,  Biochem.   Jour., 

1913,  vol.  7,  pp.  410-428. 

10  Walpole,  G.  S.,  An  improved  hydrogen  electrode,  Biochem.  Jour., 

1914,  vol.  8,  pp.  131-133. 

11  Wilke,  E.,  Ueber  eine  neue  Wasserstoffelektrode  und  ihre  Ver- 
wendbarkeit,  Zeitschr.  f.  Electrochem.,  1913,  vol.  19,  pp.  857-858. 

B.  GENERAL  METHODS. 

12  Baragiola,    W.    I.,    Concentration    of    hydrogen    ions,    Schweiz. 
Apoth.  Ztg.,  1914,  vol.  52,  pp.  641-643,  quoted  from  Chemical  Abstr., 

1915,  vol.  9,  p.  349. 

is  Bjerrum,  N.,  Die  Theorie  der  alkalimetrischen  und  azidi- 
metrischen  Titrierungen,  Sammlung  chem.  u.  chem.-tech.  Vortrage, 
1914,  vol.  21,  pp.  1-128. 

i*  Bottger,  W.,  Die  Anwendung  des  Elektrometers  als  Indikator 
beim  Titrieren  von  Sauren  und  Basen,  Zeitschr.  phys.  Chem.,  1897, 
vol.  24,  p.  253. 

is  Crozier,  W.  J.,  Eogers,  W.  B.,  and  Harrison,  B.  I.,  Methods 
employed  for  determining  the  hydrogen-ion  concentration  in  body 
fluids,  Surg.,  Gyn.,  and  Obstet.,  1915,  vol.  21,  pp.  722-727. 

is  Czepinski,  V.,  Einige  Messungen  an  Gasketten,  Zeitschr.  f. 
anorg.  Chem.,  1902,  vol.  30,  pp.  1-17. 

17  Denham,  H.  G.,  The  electrometric  determination  of  the  hydrol- 
ysis of  salts,  Jour.  Chem.  Soe.,  London,  1908,  vol.  93,  pp.  41-63. 


1919]     Schmidt-H&agland:  Table  of  PH,  H+  mid  OR-  Values    45 

is  Denham,  H.  G.,  Anomalous  behavior  of  the  hydrogen  electrode 
in  solutions  of  lead  salts,  and  the  existence  of  univalent  lead  ions  in 
aqueous  solutions,  Jour.  Chem.  Soc.,  London,  1908,  vol.  93,  pp.  424- 
427. 

is  Desha,  L.  J.,  and  Acree,  S.  F.,  On  difficulties  in  the  use  of  the 
hydrogen  electrode  in  the  measurement  of  the  concentration  of  hydro- 
gen ions  in  the  presence  of  organic  compounds,  Am.  Chem.  Jour., 
1911,  vol.  46,  pp.  638-648. 

20  Enklaar,   J.   E.,   Eine   storende   Wirkung   der   Gaselektrode   bei 
der  Bestimmung  der  Wasserstoffionenkonzentration  durch  electrische 
Messung.,  Chem.  Zentralbl.,  1910,  vol.  14,  p.  852. 

21  Pox,  C.  J.  J.,  On  the  constancy  of  the  hydrogen  gas  electrode, 
Chem.  News,  1909,  vol.  100,  p.  161. 

22  Haas,  A.  B.  C.,  A  simple  and  rapid  method  of  studying  respira- 
tion   by   the   detection   of   exceedingly   minute   quantities    of    carbon 
dioxide,  Science,  n.s.,  1916,  vol.  44,  pp.  105-108. 

23  Hasselbalch,     K.     A.,     Elektrometrische     Eeaktionsbestimmung 
kohlensaurehaltiger   Fliissigkeiten,   Biochem.   Zeitschr.,   1910,  vol.   30, 
pp.  317-331. 

24  Hasselbalch,  K.  A.,  Determination  electrometrique  de  la  reaction 
des  liquides  renfermant  de  1'acide  carbonique,  C.-E.  Lab.  Carlsberg, 
1911,  vol.  10,  pp.  69-84. 

25  Hasselbalch,  K.  A.,  Methods  for  the  electrometrie  determination 
of  the  concentration  of  hydrogen  ions  in  biological  fluids,  Biochem. 
Bull.,  1912-1913,  vol.  2,  pp.  367-372. 

26  Hasselbalch,    K.    A.,    Verbesserte    Methodik    bei    der    elektro- 
metrischen  Eeaktionsbestimmung  biologischer  Fliissigkeiten,  Bioehem. 
Zeitschr.,  1913,  vol.  49,  pp.  451-457. 

27  Hildebrand,  J.  H.,  Some  applications  of  the  hydrogen  electrode 
in  analysis,  research  and  teaching,  Jour.  Am.  Chem.  Soc.,  1913,  vol. 
35,  pp.  847-871. 

28  Kistiakowsky,  W.,  Zur  Methodik  der  Messung  von  Elektroden- 
potentialen,  Zeitschr.  f.  Elektrochem.,  1908,  vol.  14,  pp.  113-121. 

29  Luuden,  H.,  Amphoteric  electrolytes,  Jour.  Biol.   Chem.,  1908, 
vol.  4,  pp.  267-288. 

so  McClendon,  J.  F.,  The  standardization  of  a  new  colorimetric 
method  for  the  determination  of  the  hydrogen  ion  concentration,  CO2 
tension,  and  CO2  and  O2  content  of  sea  water,  of  animal  heat,  and 
of  CO2  of  the  air,  with  a  summary  of  similar  data  on  biocarbonate 
solutions  in  general,  Jour.,  Biol.  Chem.,  1917,  vol.  30,  pp.  265-288. 

si  McClendon,  J.  F.,  Shedlov,  A.,  and  Thomson,  W.,  Tables  for 
finding  the  alkaline  reserve  of  blood  serum,  in  health  and  in  acidosis, 
from  the  total  CO2  or  the  alveolar  CO2  or  the  PH  at  known  CO2  ten- 
sion, Jour.  Biol.  Chem.,  1917,  vol.  31,  pp.  519-525. 

32  Michaelis,  L.,  Die  Wasserstoffionenkonzentration.  Ihre  Bedeut- 
ung  fur  die  Biologic  und  die  Methoden  ihrer  Messung.,  210  pp., 
Berlin,  J.  Springer,  1914. 

ssMuller,  P.  T.,  et  Allemandet,  H.,  Sur  une  Electrode  a  alcali, 
Jour.  Chim.  Phys.,  1907,  vol.  5,  pp.  532-556. 

s^Noyes,  A.  A.,  Eeport  of  the  Committee  on  standard  methods 
for  determining  small  hydrogen-ion  concentrations,  8th  Intern.  Cong. 
Appl.  Chem.,  1912,  vol.  25,  pp.  95-96. 


46     University  of  California  Publications  in  Physiology     [VOL.  5 

ss  Osterhout,  W.  J.  V.,  and  Haas,  A.  E.  C.,  A  simple  method  of 
measuring  photosynthesis,  Science,  n.s.,  1918,  vol.  47,  pp.  420-422. 

36  Ringer,  W.  E.,  The  rapid  measurement  of  the  hydrogen  ion  con- 
centration of  liquids,  Chem.  Weekblad.,  vol.   8,  pp.   293-295,  quoted 
from  Chemical  Abstr.,  1911,  vol.   5,  p.   3364. 

37  Schmidt,  C.  L.  A.,  Table  of  H+  and  OH"  concentrations  corre- 
sponding  to   electromotive   forces   determined   in   gas-chain   measure- 
ments, Univ.  Calif.  Publ.  Physiol.,  1909,  vol.  3,  pp.   101-113. 

38  Sorensen,    S.    P.   L.,   Ueber    die   Messung   und    Bedeutung    der 
Wasserstoffionenkonzentration  bei  biologischen  Prozessen,  Ergeb.   d. 
Physio!.,  1912,  vol.  12,  pp.  393-532. 

39  Symes,  W.  L.,  Graphic  approximation  to  the  value  of  Sorensen 's 
PH  in  terms  of  its  integral  part,  Jour.  Physiol.,  1916,  vol.  50,  Proc. 
Physiol.  Soc.,  pp.  xxx-xxxi. 

40  Wagner,  E.  J.,  Estimation  of  the  hydrion  concentration  of  very 
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C.  THEOEETICAL. 

41  Abegg,    E.,    and    Bose,    E.,    Ueber    den    Einfluss    gleichioniger 
Zusatze   auf    die   elektromotorische   Kraft   von   Konzentrationsketten 
und  auf  die  Diff usionsgeschwindigkeit ;  Neutralsalzwirkung,  Zeitschr. 
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42  Auerbach,  F.,  Die  Potentiale  der  wichtigsten  Bezugselektroden, 
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43  Clarke,  W.  F.,  Myers.,  C.  N.,  and  Acree,  S.  F.,  A  study  of  the 
hydrogen  electrode,  of  the  calomel  electrode  and  of  contact  potential, 
Jour.  Phys.  Chem.,  1916,  vol.  20,  pp.  243-265. 

44  Ellis,  J.  H.,  The  free  energy  of  hydrochloric  acid  in  aqueous 
solution,  Jour.  Am.  Chem.  Soc.,  1916,  vol.  38,  pp.  737-762. 

45  Eucken,  A.,  Ueber  den  stationaren  Zustand  zwischen  polarisier- 
ten  Wasserstoffelektroden,  Zeitschr.  f.  physik.  Chem.,  1907,  vol.  59, 
pp.  72-117. 

46  Freundlich,  H.,  and  Makelt,  E.,  Ueber  den  absoluten  Nullpunkt 
des  Potentials,  Zeitschr.  f.  Electrochem.,  1909,  vol.  15,  pp.  161-165. 

47  Glaser,    L.,    Studien   iiber    die   elektrolytische   Zersetzung   wass- 
riger  Losungen,  Zeitschr.  f.  Electrochem.,  1898,  vol.  4,  pp.  355-359, 
373-379,  424-428. 

48  Goodwin,    H.    M.,    Studien    zur    voltaschen    Kette,    Zeitschr.    f. 
physik.  Chem.,  1894,  vol.  13,  pp.  577-656. 

49  Hardman,  E.   T.,  and  Lapworth,  A.,   Electromotive   forces   in 
alcohol.     II,  The  hydrogen  electrode  in  alcohol  and  the  influence  of 
water   on  its  electromotive   force,  Jour.   Chem.   Soc.,   London,   1911, 
vol.  99,  pp.  2242-2253. 

so  Hardman,  E.  T.,  and  Lapworth,  A.,  Electromotive  forces  in 
alcohol.  Ill,  Further  experiments  with  the  hydrogen  electrode  in 
dry  and  moist  hydrogen  chloride,  Jour.  Chem.  Soc.,  London,  1912, 
vol.  101,  pp.  2249-2255. 

si  Harned,  H.  S.,  The  hydrogen-  and  hydroxyl-ion  activities  of 
solutions  of  hydrochloric  acid,  sodium  and  potassium  hydroxides  in 
the  presence  of  neutral  salts,  Jour.  Am.  Chem.  Soe.,  1915,  vol.  37, 
pp.  2460-2482. 


1919]     Schmidt-Hoagland:  Table  of  PH,  H+  and  OH-  Values     47 

52  Harned,  H.  S.,  The  hydrogen  and  chlorine  ion  activities  of  solu- 
tions of  potassium  chloride  in  0.1  molal  hydrochloric  acid,  Jour.  Am. 
Chem.  Soc.,  1916,  vol..  38,  pp.  1986-1995. 

ss  Henderson,  L.  J.,  A  diagrammatic  representation  of  equilibria 
between  acids  and  bases  in  solution,  Jour.  Am.  Chem.  Soc.,  1908, 
vol.  30,  pp.  954-960. 

s*  Henderson,  P.,  Zur  Thermodynamik  der  Fliissigkeitsketten, 
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55  Henderson,  P.,  Zur  Thermodynamik  der  Fliissigkeitsketten, 
Zeitschr.  phys.  Chem.,  1908,  vol.  63,  pp.  325-345. 

se  Kanolt,  C.  W.,  louization  of  water  at  0°,  18°,  and  25°  derived 
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57  Le  Blanc,  M.,  Die  elektromotorischen  Krafte  der  Polarization, 
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ss  Lewis,  G.  N.,  Die  Bestimmung  der  lonenhydratation  durch 
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ss  Lewis,  G.  N.,  The  activity  of  the  ions  and  the  degree  of  disso- 
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so  Lewis,  G.  N.,  and  Eandall,  M.,  The  free  energy  of  oxygen,  hydro- 
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si  Lewis,  G.  N.,  Brighton,  T.  B.,  and  Sebastian,  E.  L.,  A  study  of 
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62  Lewis,  W.  K.,  Eine  Methode  zur  Berechnung  von  lonenkonzen- 
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es  Loomis,  N.  E.,  and  Acree,  S.  F.,  A  study  of  the  hydrogen 
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64  Loomis,  N.  E.,  and  Acree,  S.  F.,  The  application  of  the  hydro- 
gen electrode  to  the  measurement  of  the  hydrolysis  of  aniline  hydro- 
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es  Loomis,  N.  E.,  and  Aeree,  S.  F.,  The  effect  of  pressure  on  the 
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67  Lorenz,  E.,  and  Bohi,  A.,  Beitrage  zur  Theorie  der  elektro- 
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48     University  of  California  Publications  in  Physiology     [VOL.  5 

70  Lowenherz,   E.,    Ueber    den    Einfluss    des    Zusatzes    von   Athyl- 
alkohol  auf  die  elektrolytische  Dissociation  des  Wassers,  Zeitschr.  f. 
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71  Michaelis,  L.,   and   Kona,   P.,   Die  Dissoziationskonstanten   ein- 
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72  Myers,  C.  N.,  and  Acree,  S.  F.,  A  study  of  the  hydrogen  elec- 
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73  Nernst,   W.,   Zur   Kinetik   der   in  Losung   befindlichen   Korper, 
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74  Nernst,  W.,  Die  electromotorische  Wirksamkeit  der  lonen,  Zeit- 
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75  Nernst,   W.,   Zur   Dissociation   des   Wassers,   Zeitschr.    f.    phys. 
Chem.,  1894,  vol.  14,  pp.  155-156. 

76  Nernst,  W.,  Ueber   die   Zahlenwerte  einiger  wichtiger   physiko- 
ehemischer  Konstanten,  Zeitsehr.  f.  Electrochem.,   1904,  vol.   10,  pp. 
629-630. 

77  Ostwald,  W.,  Die  Dissociation   des   Wassers,   Zeitschr.   f.   phys. 
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78  Ostwald,  W.,  Ueber  die  absoluten  Potentiale  der  Metalle  nebst 
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79  Poma,  G.,  Neutralsalzwirkung  und  Zustand  der  lonen  in  Losung, 
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so  Poma,  G.,  and  Patroni,  A.,  Einfluss  der  Neutralsalze  auf  den 
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pp.  196-214. 

si  Eothmund,  V.,  Die  Potentialdifferenzen  zwischen  Metallen  und 
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82  Sackur,   O.,   Ueber   den  Einfluss   gleiehioniger   Zusatze   auf   die 
elektromotorische  Kraft  von  Fliissigkeiten .   Ein  Beitrag  zur  Kennt- 
nis  des  Verhaltens  starker  Elektrolyte,  Zeitschr.  f.  phys.  Chem.,  1901, 
vol.  38,  pp.  129-162. 

83  Smale,  F.  J.,  Studien  iiber  Gasketten,  Zeitschr.  f .  physik.  Chem., 
1894,  vol.  14,  pp.  577-621. 

s*  Tolman,  E.  C.,  and  Greathouse,  L.  H.,  The  concentration  of 
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ss  Wilsmore,  N.  T.  M.,  .Ueber  Elektroden-potentiale,  Zeitschr.  f . 
phys.  Chem.,  1900,  vol.  35,  pp.  291-332. 

86  Wilsmore,  N.  T.  M.,  and  Ostwald,  W.,  Ueber  Elektrodenpoten- 
tiale  und  absolute  Potentiale,  Zeitschr.  f.  phys.  Chem.,  1901,  vol.  36, 
pp.  91-98. 

D.  CONTACT  POTENTIAL. 

87  Abegg,  E.,  and  Gumming,  A.  C.,  Zur  Eliminierung  der  Fliissig- 
keitspotentiale,  Zeitschr.  f.  Electrochem.,  1907,  vol.  13,  pp.  17-18. 

ss  Bjerrum,  N.,  Ueber  die  Giiltigkeit  der  Planckschen  Formel  fur 
das  Diffusionspotential,  Zeitschr.  f.  Electrochem.,  1911,  vol.  17,  pp. 
58-61. 


1919]     Schmidt-Hoagland:  Table  of  PH,  H+  and  OH~  Values     49 

89  Bjerrum,  N.,  Ueber  die  Elimination  des  Fliissigkeitspotentials 
bei  Messungen  von  Elektrodenpotentialen,  Zeitsehr.   f.  Electrochem., 
1911,  vol.  17,  pp.  389-393. 

90  Bjerrum,    N.,    Ueber    die    Elimination    des    Diffusionspotentials 
zwischen   verdiinnten   wasserigen   Losungen   durch   Einschalten   einer 
konzentrierten  Chlorkaliumlosuug,  Zeitsehr.  f.  phys.  Chem.,  1905,  vol. 
53,  p.  428. 

si  Chanoz,  A.  M.,  Eecherches  experimentales  sur  les  contacts 
liquides,  Ann.  de  1'Universite  de  Lyon,  1906,  no.  18,  pp.  1-99. 

92  Gumming,   A.    C.,   The   elimination   of   potential    due   to    liquid 
contact,  Trans.  Faraday  Soc.,  1906,  vol.  2,  pp.  213-221. 

93  Gumming,  A.  C.,  A  simple  equation  for  the  calculation  of  the 
diffusion  potential,  Trans.  Faraday  Soc.,  1912,  vol.  8,  pp.  86-93. 

94  Gumming,  A.  C.,  and  Gilchrist,  E.,  The  effect  of  variations  in 
the  nature  of  the  liquid  boundary  on  the  electromotive  force,  Trans. 
Faraday  Soc.,  1913,  vol.  9,  pp.  174-185. 

95  Johnson,    K.    E.,    Zur    Nernst-Planckschen    Theorie    iiber    die 
Potentialdifferenz   zwischen   verdiinnten   Losungen,   Ann.    d.   Physik., 
1904,  (4),  vol.  4,  pp.  995-1003. 

96  Lewis,  G.  N.,  and  Sargent,  L.  W.,  Potentials  between  liquids, 
Jour.  Am.  Chem.  Soc.,  1909,  vol.  31,  pp.  363-367. 

97  Negbaur,  W.,  Experimentaluntersuchungen  iiber  Potentialdiffer- 
enzen  an   den  Beriihrungsflachen   sehr   verdiinnter  Losungen,  'Wiede- 
mann's Ann.  d.  Phys.  u.  Chem.,  1891,  N.F.,  vol.  44,  pp.  737-758. 

98  Planck,  M.,  Ueber  die  Erregung  von   Electricitat  und  Warme 
in  Electrolyten,   Wiedemann's   Ann.   d.  Phys.  u.   Chem.,   1890,   N.F., 
vol.  39,  pp.  161-186. 

99  Planck,    M.,    Ueber    die    Potentialdifferenz    zwischen    zwei    ver- 
diinnten Losungen  binarer  Electrolyte,  Wiedemann's  Ann.   d.   Phys. 
u.  Chem.,  1890,  N.F.,  vol.  40,  pp.  561-576. 

100  Tower,  O.  F.,  Ueber  Potentialdifferenzen  an  den  Beriihrungs- 
nachen verdiinnter  Losungen,  Zeitsehr.  f.  phys.  Chem.,  1896,  vol.  20, 
pp.  198-206. 

E.  CALOMEL  ELECTEODE8 

101  Coggeshall,  G.  W.,  Ueber  die  Konstanz  der  Kalomelelektrode, 
Zeitsehr.  f.  phys.  Chem.,  1895,  vol.  17,  pp.  62-86. 

102  Desha,  L.   J.,  An  apparatus  for  the   purification  of  mercury, 
Am.  Chem.  Jour.,  1909,  vol.  41,  pp.  152-155. 

103  Hildebrand,  J.  H.,  Purification  of  mercury,  Jour.  Am.  Chem. 
Soc.,  1909,  vol.  31,  pp.  933-935. 

i04Hulett,  G.  A.,  and  Minchin,  H.  D.,  The  distillation  of  amal- 
gams and  the  purification  of  mercury,  Physical  Eev.,  1905,  vol.  21, 
pp.  388-398. 

105  Lipscomb,  G.  F.,  and  Hulett,  G.  A.,  A  calomel  standard  cell, 
Jour.  Am.  Chem.  Soc.,  1916,  vol.  38,  p.  20. 

ice  Loomis,  N.  E.,  Notes  upon  the  potentials  of  calomel  and 
hydrogen  electrodes,  Jour.  Phys.  Chem.,  1915,  vol.  19,  pp.  660-664. 

107  Palmaer,  W.,  Ueber  das  absolute  Potential  der  Kalomelelek- 
trode, Zeitsehr.  f.  phys.  Chem.,  1907,  vol.  59,  pp.  129-191. 

108  Palmaer,  W.,  Ueber  das  absolute  Potential  der  Kalomelelek- 
trode, Zeitsehr.  f.  Electrochem.,  1903,  vol.  9,  pp.  754-757. 


50     University  of  California  Publications  in  Physiology     [VOL.  5 

109  Eichards,  T.  W.,  TJeber  den  Temp&raturkoeffizienten  des  Poten- 
tials der  Kalomelelektrode  mit  verschiedenen  gelosten  Elektrolyten, 
'  Zeitschr.  f.  phys.  Chem.,  1897,  vol.  24,  pp.  39-54. 

no  Sauer,  L.,  Bezugselektroden,  Zeitschr.  f.  phys.  Chem.,  1904, 
vol.  47,  pp.  146-184. 


F.  BUFFER  MIXTURES. 

111  Clark,  W.  M.,  and  Lubs,  L.  A.,  Hydrogen  electrode  potentials 
of  phthalate,  phosphate,  and  borate  buffer  mixtures,  Jour.  Biol.  Chem., 
1916,  vol.  25,  pp.  479-510. 

112  Koppel,  M.,  and  Spiro,  K.,  Ueber  die  Wirkung  von  Moderatoren 
(Puffern)    bei   der   Verschiebung   des   Saure-Basengleichgewichtes   in 
biologischen  Fliissigkeiten,  Biochem.  Zeitschr.,  1914,  vol.  65,  pp.  409- 
439. 

us  Palitzsch,  S.,  Ueber  die  Anwerdung  von  Borax-  und  Bor- 
saurelosungen  bei  der  eolorimetrischen  Messung  der  Wasserstoffionen- 
konzentration  des  Meerwassers,  Biochem.  Zeitschr.,  1915,  vol.  70,  pp. 
333-343. 

114  Palitzsch,  S.,  Sur  1'emploi  de  solutions  de  borax  et  d'acide 
borique  dans  la  determination  colorimetrique  de  la  concentration  en 
ions  hydrogene  de  1'eau  de  mer,  C.-R.  Lab.  Carlsberg,  1916,  vol.  11, 
pp.  199-211. 

us  Prideaux,  E.  B.  R.,  The  sodium  phosphate  standards  of  acidity, 
Biochem.  Jour.,  1911,  vol.  6,  pp.  122-126. 

lie  Prideaux,  E.  B.  R.,  On  the  use  of  partly  neutralized  mixtures 
of  acids  as  hydrion  regulators,  Proc.  Royal  Soe.,  London  (A),  1916, 
vol.  92,  pp.  463-468. 

117  Ringer,  W.  E.,  The  concentration  of  hydrogen  ions  in  dilute 
solutions  of  phosphoric  acid,  mono-  and  disodium  phosphate,  Chem. 
Weekblad,  vol.  6,  pp.  446-452,  quoted  from  Chemical  Abst.,  1910, 
vol.  4,  pp.  5-6. 

us  Schmidt,  C.  L.  A.,  and  Finger,  C.  P.,  Potential  of  a  hydrogen 
electrode  in  acid  and  alkaline  solutions,  Jour.  Phys.  Chem.,  1908, 
vol.  12,  pp.  406-416. 

us  Walpole,  G.  S.,  The  effect  of  dilution  on  the  hydrogen  poten- 
tials of  acetic  acid  and  ' '  standard  acetate ' '  solutions,  Jour.  Chem. 
Soc.,  London,  1914,  vol.  105,  pp.  2521-2529. 

120  Walpole,  G.  S.,  Hydrogen  potentials  of  mixtures  of  acetic  acid 
and  sodium  acetate,  Jour.  Chem.   Soc.,  London,  1914,  vol.   105,  pp. 
2501-2520. 

121  Walpole,  G.  S.,  Notes  on  regular  mixtures,  recent  indicators, 
etc.     II,  Biochem.  Jour.,  1914,  vol.  8,  pp.  628-640. 

G.  MISCELLANEOUS  ELECTRODES. 

122  Bancroft,  W.,  Ueber  Oxydationsketten,  Zeitschr.  f .  phys.  Chem., 
1892,  vol.  10,  pp.  387-409. 

123  Bose,  E.,  Untersuchungen  uber  die  elektromotorische  Wirksam- 
keit  der  elementaren  Gase,  Zeitschr.  f.  phys.  Chem.,  1900,  vol.   34, 
pp.  700-760. 


Schniidt-Hoagland:  Table  of  PH,  H+  and  OH-  Values     51 

124  Bose,  E.,  Untersuehungen  iiber  die  elektromotorische  Wirksam- 
keit  der   elementaren   Gase,  Zeitsehr.   f.   phys.   Chem.,   1901,   vol.   38, 
pp.  1-26. 

125  Brislee,    F.    J.,    The    potential    of    the    hydrogen-oxygen    cell, 
Trans.  Faraday  Soc.,  1905,  vol.  1,  pp.  65-74. 

126  Brb'nsted,  J.  N.,  Die  electromotorische  Kraft  der  Knallgaskette, 
Zeitsehr.  f.  phys.  Chem.,  1908,  vol.  65,  pp.  84-92. 

127  Hoeper,    V.,    Ueber    die    elektromotorische    Wirksamkeit    des 
Kohlenoxyd -gases,  Zeitsehr.  f.  anorg.  Chem.,  1899,  vol.  20,  pp.  419- 
451. 

128  Lapworth,  A.,  and  Partington,  J.  E.,  Electromotive  forces  in 
alcohol.     I,  Concentration  cells  with  electrodes  reversible  to  chlorine 
ions,  Jour.  Chem.  Soc.,  London,  1911,  vol.  99,  pp.  1417-1427. 

120  Laurie,  A.  P.,  Die  elektromotorische  Kraft  von  lodkonzentra- 
tionsketten  in  Wasser  und  Alkohol,  Zeitsehr.  phys.  Chem.,  1908,  vol. 
64,  pp.  615T628. 

iso  Lewis,  G.  N.,  and  Sargent,  L.  W.,  The  potential  of  the  f erro- 
ferricyanide  electrode,  Jour.  Am.  Chem.  Soc.,  1909,  vol.  31,  pp.  355- 
363. 

isi  Lewis,  G.  N.,  and  Eupert,  F.  F.,  The  potential  of  the  chlorine 
electrode,  Jour.  Am.  Chem.  Soc.,  1911,  vol.  33,  pp.  299-307. 

132  Lorenz,  E.,  Die  Oxydtheorie  der  Sauerstoffelektrode,  Zeitsehr. 
f.  Electrochem.,  1908,  vol.  14,  pp.  781-783. 

iss  Luther,  E.,  and  Michie,  A.  C.,  Das  elektromotorisehe  Verhalten 
von  Uranyl-Uranogemengen,  Zeitsehr.  f.  Electrochem.,  1908,  vol.  14, 
pp.  826-829. 

is*  Maitland,  W.,  Ueber  das  lod-Potential  und  das  Ferri-Ferro- 
Potential,  Zeitsehr.  f.  Electrochem.,  1906,  vol.  12,  pp.  263-268. 

iss  Miiller,  E.,  Die  elektromotorische  Kraft  der  Chlorknallgaskette, 
Zeitsehr.  f.  phys.  Chem.,  1902,  vol.  40,  pp.  158-168. 

136  Naumann,   E.,   Die   elektromotorische   Kraft    der    Cyanwasser- 
stoffkette,  Zeitsehr.  f.  Elektroehem.,  1910,  vol.  16,  pp.  191-199. 

137  Nernst,   W.,   and   Sand,   J.,   Zur   Kenntnis   der    unterchlorigen 
Saure.     Elektromotorisches  Verhalten,  Zeitsehr.  f.  phys.  Chem.,  1904, 
vol.  48,  pp.  601-609. 

138  Nernst,    W.,    and    Wartenberg,    H.    v.,    Die    Dissociation    von 
Wasserdampf,  Zeitsehr.  phys.  Chem.,  1906,  vol.  56,  pp.  513-547. 

139  Neumann,  B.,  Ueber  das  Potential  des  Wasserstoffs  und  einiger 
Metalle,  Zeitsehr.  f.  phys.  Chem.,  1894,  vol.  14,  pp.  193-230. 

140  Peters,  E.,  Ueber  Oxydations-  und  Eeduktions-ketten  und  den 
Einfluss  komplexer  lonen  auf  ihre  elektromotorische  Kraft,  Zeitsehr. 
f.  phys.  Chem.,  1898,  vol.  26,  pp.  193-236. 

141  Preuner,    G.,    Ueber    die    Dissociationskonstante    des    Wassers 
und  die  elektromotorische  Kraft  der  Knallgaskette,  Zeitsehr.  f.  phys. 
Chem.,  1902,  vol.  42,  pp.  50-58. 

142  Schoch,  E.  P.,  A  study  of  reversible  oxidation  and  reduction 
reactions  in  solutions,  Jour.  Am.  Chem.  Soc.,  1904,  vol.  26,  pp.  1422- 
1433. 

143  Sehoch,  E.  P.,  The  potential  of  the  oxygen  electrode :  a  report 
of  progress,  Jour.  Phys.  Chem.,  1910,  vol.  14,  pp.  665-677. 


52     University  of  California  Publications  in  Physiology     [VOL.  5 

II.  BIOLOGICAL. 
A.  BLOOD. 

144  Abel,   E.,   and   Fiirth,    O.    v.,   Zur    physikalisehen   Chemie    des 
Oxyhamoglobins.      Das   Alkalibindungsvermogen    des   Blutfarbstoffes, 
Zeitschr.  f.  Electrochem.,  1906,  vol.  12,  pp.  349-359. 

145  Aggazzotti,   A.,   La   reazione    de   sangue   nell'    aria   rarefatta 
determinata  coi  metodi  titolimetrici  ed  elettrometrici,  Atti  d.  Eeale 
Accad.  d.  Lincei,  Eome,  1906,  vol.  15,  pp.  474-483. 

146  Benedict,   H.,   Der   Hydroxylionengehalt   des   Diabetikerblutes, 
Arch.  f.  d.  ges.  Physiol.,  1906,  vol.  115,  pp.  106-117. 

147  Bugarszky,   S.,  and  Tangl,  F.,  Physikalisch-cliemische   Unter- 
suchungen  iiber  die  moleculareu  Concentrationsverhiiltnisse  des  Blut- 
serums, Arch.  f.  d.  ges.  Physiol.,  1898,  vol.  72,  pp.  531-565. 

148  Corral,    J.    M.,    Ueber    die    elektrometrische    Bestimmung    der 
wahren   Eeaktion   des   Blutes,  Biochem.   Zeitschr.,   1915,   vol.   72,   pp. 
1-25. 

149  Cullen,  G.  E.,  The .  electrometric  titration  of  plasma  as  a  meas- 
ure of  its  alkaline  reserve,  Jour.  Biol.  Chem.,  1917,  vol.  30,  pp.  369- 
388. 

iso  Farkas,  G.,  Ueber  die  Concentration  der  Hydroxylionen  im 
Blutserum,  Arch.  f.  d.  ges.  Physiol.,  1903,  vol.  98,  pp.  551-576. 

is1  Farkas,  G.,  and  Scipiades,  E..  Ueber  die  molekularen  Concen- 
trations-verhaltnisse  des  Blutserums  der  Schwangeren,  Kreissenden 
und  Wochnerinnen  und  des  Fruchtwassers,  Arch.  f.  d.  ges.  Physiol., 
1903,  vol.  98,  pp.  577-587. 

152  Fraenckel,  P.,  Eine  neue  Methqde  zur  Bestimmung  der  Re- 
action des  Blutes,  Arch.  f.  d.  ges.  Physiol.,  1903,  vol.  96,  pp.  601-623. 

iss  Friedenthal,  H.,  Ueber  die  Eeaktion  des  Blutserums  der  Wirbel- 
tiere  und  die  Eeaktion  der  lebendigen  Substantz  im  allgemeinen, 
Zeitschr.  f.  allgemeine  Physiol.,  1902,  vol.  1,  pp.  56-66. 

154  Friedenthal,  H.,  Reactionsbestimmungen  im  natiirlichen  Serum 
und    iiber    Herstellung    einer    zum    Ersatz    des    natiirlichen    Serums 
geeigneten  Salzlosung,  Arch.  Anat.  u.  Physiol.   (Physiol.  Abt.),  1903, 
pp.  550-554. 

155  Friedenthal,  H.,  Ueber  die  Eeaktion  des  Blutserums  der  Wirbel- 
tiere    und    die    Eeaktion    der    lebendigen    Substanz    im    allgemeinen, 
Zeitschr.,  f.  allgemeine  Physiol.,  1904,  vol.  4,  pp.  44-61. 

iss  Hasselbalch,  K.  A.,  The  reduced  and  the  regulated  "hydrogen 
figure"  of  the  blood,  Biochem.  Zeitschr.,  1916,  vol.  74,  pp.  56-62, 
quoted  from  Physiol  Abst.,  1916,  vol.  1,  p.  252. 

!57  Hasselbalch,  K.  A.,  The  calculation  of  the  hydrogen  number 
of  the  blood  from  the  free  and  bound  carbon  dioxide  of  the  same,  and 
the  binding  of  oxygen  by  the  blood  as  a  function  of  the  hydrogen 
number,  Biochem.  Zeitschr.,  1916,  vol.  78,  pp.  112-144,  quoted  from 
Chem.  Abst,  1917,  vol.  11,  pp.  1656-1657. 

iss  Hasselbalch,  K.  A.,  The  true  nature  of  the  "acidotic  condi- 
tion" of  infants,  Biochem.  Zeitschr.,  1917,  vol.  80,  pp.  251-258, 
quoted  from  Chem.  Abst.,  1917,  vol.  11,  p.  2693. 

iss  Hasselbalch,  K.  A.,  and  Gammeltoft,  S.  A.,  Die  Neutralitats- 
regulation  des  graviden  Organismus,  Biochem.  Zeitschr.,  1914,  vol.  68, 
pp.  206-264. 


1919]     Schmidt-Hoagland:  Table  of  PH,  H+  and  OH-  Values     53 

160  Hasselbalch,  K.  A.,  and  Lundsgaard,  C.,  Blutreaktion  und 
Lungenventilation,  Skand.  Arch.  f.  Physiol.,  1912,  vol.  27,  pp.  13-31. 

lei  Hasselbalch,  K.  A.,  and  Lundsgaard,  C.,  Elektrometrische 
Eeaktionsbestimmung  des  Blutes  bei  Korpertemperatur,  Biochem. 
Zeitschr.,  1912,  vol.  38,  pp.  77-91. 

102  Henderson,  L.  J.,  On  the  neutrality  equilibrium  in  blood  and 
protoplasm,  Jour.  Biol.  Chem.,  1909,  vol.  7,  pp.  29-35. 

IBS  Hober,  E.,  Ueber  die  Hydroxylionen  des  Blutes,  Arch,  f .  d.  ges. 
Physiol.,  1900,  vol.  81,  pp.  522-539. 

16*  Hober,  E.,  Ueber  die  Hydroxylionen  des  Blutes,  Arch,  f .  d.  ges. 
Physiol.,  1903,  vol.  99,  pp.  572-593. 

les  Hober,  E.,  Die  Gaskettenmethode  zur  Bestimmung  der  Blut- 
reaktion, Deut.  med.  Woch.,  1917,  vol.  43,  pp.  551-552. 

166  Homer,  A.,  A  note  on  the  Use  of  indicators  for  the  colori- 
metric  determination  of  the  hydrogen  ion  concentration  of  sera,  Bio- 
chem. Jour.,  1917,  vol.  11,  pp.  283-291. 

i6r  Konikoff,  A.  P.,  Ueber  die  Bestimmung  der  wahren  Blutreak- 
tion mittels  der  elektrischen  Methode,  Biochem.  Zeitschr.,  1913,  vol. 
51,  pp.  200-210. 

168  Kreibich,     C.,     Ueber     die     Hydroxylionenkonzentration     des 
pathologischen  Blutes,  Wien.  klin.  Woch.,  1910,  vol.  23,  pp.  355-358; 

1911,  vol.  24,  pp.  1419-1420. 

169  Levy,  E.  L.,  Eowntree,  L.  G.,  and  Marriott,  W.  M.,  A  simple 
method  for  determining  variations  in  the  hydrogen-ion  concentration 
of  the  blood,  Arch.  Int.  Med.,  1915,  vol.  16,  pp.  389-405. 

i^o  Lundsgaard,  C.,  Die  Eeaktion  des  Blutes,  Biochem.  Zeitschr., 

1912,  vol.  41,  pp.  247-267. 

171  Masel,  J.,  Zur  Frage  der  Saurevergiftung  beim  Coma  diabeti- 
cum,  Zeitschr.  f.  klin.  Med.,  1914,  vol.  79,  pp.  1-12. 

172  McClehdon,  J.  F.,  Improved  gas  chain  methods  of  determining 
hydrogen  ion  concentration  in  blood,  Jour.  Biol.  Chem.,  1916,  vol.  24, 
pp.  519-526. 

173  McClendon,  J.  F.,  A  new  hydrogen  electrode  for  the  electro- 
metric  titration  of  the  alkaline  reserve  of  blood  plasma  and  other 
frothing  fluids,  Jour.  Biol.  Chem.,  1918,  vol.  33,  pp.  19-29. 

17*  Menten,  M.  L.,  and  Crile,  G.  W.,  Studies  on  the  hydrogen-ion 
concentration  in  blood  under  various  abnormal  conditions,  Am.  Jour. 
Physiol.,  1915,  vol.  38,  pp.  225-232. 

175  Michaelis,  L.,  Die   Bedeutung  des  Wasserstoffionenkonzentra- 
tion  des  Blutes  und  der  Gewebe,  Deut.  med.  Woch.,  1914,  vol.   40, 
pp.  1170-1171. 

176  Miehaelis,  L.,  and  Davidoff,  W.,  Methodisches  und  Sachliches 
zur    elektrometrischen    Bestimmung    der    Blutalkalescenz,    Biochem. 
Zeitschr.,  1912,  vol.  46,  pp.  131-150. 

!77  Michaelis,  L.,  and  Eona,  P.,  Electrochemische  Alkalinitats- 
messungen  an  Blut  und  Serum,  Biochem.  Zeitschr.,  1909,  vol.  18, 
pp.  317-339. 

178  Milroy,  T.  H.,  Changes  in  the  hydrogen  ion  concentration  of 
the   blood  produced  by   pulmonary  ventilation,   Quar.    Jour.   Exper. 
Physiol.,  1914,  vol.  8,  pp.  141-153. 

179  Palmer,   W.    W.,   and    Henderson,   L.    J.,    Clinical    studies    on 
acid  base  equilibrium  and  the  nature  of  acidosis,  Arch.  Int.  Med., 

1913,  vol.  12,  pp.  153-170. 


54     University  of  California  Publications  in  Physiology     [VOL.  5 

iso  Peters,  E.  A.,  A  combined  tonometer  and  electrode  cell  for 
measuring  the  H-ion  concentration  of  reduced  blood  at  a  given  ten- 
sion of  CO2,  Jour.  Physiol.,  Proc.  Physiol.  Soc.,  1914,  vol.  48,  pp. 
vii,  viii. 

181  Pfaundler,    M.,    Ueber    die    actuelle    Reaction    des    kindlichen 
Blutes,  Arch.  v.  Kinderheilk.,  1905,  vol.  41,  pp.  161-184. 

182  Porges,  O.,  The  ' '  reduced ' '  and  ' '  regulated ' '  hydrogen  num- 
ber of  the  blood,  Biochem.  Zeit.,  1916,  vol.  77,  pp.   241-248,  quoted 
from  Physiol.  Abst.,  1917,  vol.  2,  pp.  32-33. 

iss  Quagliariello,  G.,  Ueber  die  Hydroxylionenkonzentration  des 
Blutes  bei  der  Temperaturerhohung  nach  dem  Warmestich,  Biochem. 
Zeitschr.,  1912,  vol.  44,  pp.  162-164. 

184  Robertson,  T.  B.,  On  the  nature  of  the  chemical  mechanism 
which  maintains  the  neutrality  of  the  tissues  and  tissue-fluids,  Jour. 
Biol.  Chem.,  1909,  vol.  6,  pp.  313-320. 

iss  Robertson,  T.  B.,  Concerning  the  relative  magnitude  of  the 
parts  played  by  the  proteins  and  by  the  bicarbonates  in  the  main- 
tenance of  the  neutrality  of  the  blood,  Jour.  Biol.  Chem.,  1910,  vol. 
7,  pp.  351-357. 

186  Roily,  F.,  Ueber  die  Reaktion  des  Blutserums  bei  normalen  und 
pathologischen  Zustanden,  Munch,  med.  Woch.,  1912,  voli  59,  pp. 
1201-1205,  1274-1277. 

IST  Rona,  P.,  and  Gyorgy,  P.,  Beitrag  zur  Frage  der  lonenverteil- 
ung  im  Blutserum,  Biochem.  Zeitschr.,  1913,  vol.  56,  pp.  416—438. 

iss  Rona,  P.,  and  Takahashi,  D.,  Beitrag  zur  Frage  nach  dem  Ver- 
halten  des  Calciums  im  Serum,  Biochem.  Zeitschr.,  1913,  vol.  49,  pp. 
370-380. 

iss  Rona,  P.,  and  Yippo,  A.,  Ueber  den  Einfluss  der  "Wasserstoff- 
ionenkonzentratioii  auf  die  Saurestoffdissoziationscurve  des  Hamo- 
globins,  Biochem.  Zeitschr.,  1916,  vol.  76,  pp.  187-217,  quoted  from 
Physiol.  Abst.,  1917,  vol.  2,  p.  32. 

190  Scott,  R.  W.,  The  effect  of  the  accumulation  of  carbon  dioxide 
on  the  tidal  air  and  on  the  H-ion  concentration  of  the  arterial  blood 
in  the  decerebrate  cat,  Am.  Jour.  Physiol.,  1917,  vol.  44,  pp.  196-211. 

191  Stillman,  E.,  Van  Slyke,  D.  D.,  Cullen,  G.  E.,  and  Fitz,  R., 
The  blood,  urine,  and  alveolar  air  in  diabetic  acidosis,  Jour.   BioL 
Chem.,  1917,  vol.  30,  pp.  405-456. 

192  Szili,  A.,   Untersuchungen   iiber    den   Hydroxylionengehalt   des 
placentaren  (fotalen)  Blutes,  Arch.  f.  d.  ges.  Physiol.,  1906,  vol.  115, 
pp.  72-81. 

193  Winternitz,  H.,  Beitrage  zur  Alkalimetrie  des  Blutes,  Zeitschr. 
f.  physiol.  Chem.,  1891,  vol.  15,  pp.  505-512. 

B.  URINE. 

194  Blatherwick,  N.  R.,  The  specific  r61e  of  foods  in  relation  to  the 
composition  of  the  urine,  Arch.  Int.  Med.,  1914,  vol.  14,  pp.  409-450. 

195  Bugarszky,    S.,   Ueber   die    molecularen    Concentrationsverhalt- 
nisse   des  normalen  menschlichen   Harns,   Arch.   f.    d.   ges.   Physiol., 
1897,  vol.  68,  pp.  389-407. 

196  Foa,  C.,  Le  reaction  de  1  'urine  et  du  sue  pancreatique  etudiee 
par  la  methode  eleetrome'trique,  C.-R.  Soe.  Biol.,  1905,  vol.  58,  pp. 
867-869. 


1919]     Schmidt-Haagland:  Table  of  PH,  H+  and  OH-  Values     55 

197  Henderson,  L.  J.,  Messungen  der  normalen  Harnaciditat, 
Biochem.  Zeitschr.,  1910,  vol.  24,  pp.  40-44. 

las  Henderson,  L.  J.,  and  Palmer,  W.  W.,  On  the  intensity  of 
urinary  acidity  in  normal  and  pathological  conditions,  Jour.  Biol. 
Chem.,  1913,  vol.  13,  pp.  393-405. 

199  Henderson,   L.   J.,   and   Palmer,   W.   W.,   On   the   extremes   of 
variation  of  the  concentration  of  ionized  hydrogen  in  human  urine, 
Jour.  Biol.  Chem.,  1913,  vol.  14,  pp.  81-85. 

200  Henderson,  L.  J.,  and  Spiro,  K.,  Ueber  Basen-  und  Sauregleich- 
gewicht  im  Harn,  Biochem.  Zeitschr.,  1908,  vol.  15,  pp.  105-113. 

201  Hober,  R.,  Die  Aciditat  des  Hams  vom  Standpunkt  der  lonen- 
lehre,  Beitr.  z.  chem.  Physiol.  u.  Path.,  1903,  vol.  3,  pp.  525-542. 

202  Howe,  P.   E.,  and   Hawk,   P.   B.,   Variations  in   the   hydrogen 
ion  concentration  of  the  urine  of  man  accompanying  fasting  and  the 
low-  and  high-protein  regeneration  periods,  Jour.  Biol.  Chem.,  Proc., 
1914,  vol.  17,  p.  xlviii. 

203  Newburgh,  L.   H.,  Palmer,  W.   W.,  and  Henderson,  L.   J.,  A 
study  of  hydrogen  ion  concentration  of  the  urine  in  heart  disease, 
Arch.  Int.  Med.,  1913,  vol.  12,  pp.  146-152. 

204  Rhorer,  L.  v.,  Die  Bestimmung  der  Harnaciditat  auf  elektro- 
metrischen  Wege,  Arch.  f.  d.  ges.  Physiol.,  1901,  vol.  86,  pp.  586-602. 

205  Ringer,  W.   E.,  Zur  Aciditat  des   Harns,   Zeitschr.   f .  physiol. 
Chem.,  1909,  vol.  60,  pp.  341-363. 

206  Ringer,  W.  E.,  Ueber  die  Bedingungen  der  Ausscheidung  von 
Harnsaure   und  harnsauren   Salzen   aus  ihren  Losungen,  Zeitschr.   f. 
physiol.  Chem.,  1910,  vol.  67,  pp.  332-403. 

207  Skramlik,  E.  v.,  Ueber  Harnaciditat,  Zeitschr.  f.  physiol.  Chem., 
1911,  vol.  71,  pp.  290-310. 

C.  MILK. 

208  Allemann,   O.,    Die   Bedeutung    der   Wasserstoffionen    f iir    die 
Milchgerinnung,  Biochem.  Zeitschr.,  1912,  vol.  45,  pp.  346-358. 

209  Clark,  W.  M.,  The  reaction  of  cow 's  milk  modified  for  infant 
feeding,  Jour.  Med.  Res.,  1915,  vol.  31,  pp.  431-453. 

210  Davidsohn,  H.,  Ueber  die  Reaktion  der  Frauenmilch,  Zeitschr. 
f.  Kinderheilk.,  1913,  vol.  9,  pp.  11-18. 

211  Foa,  C.,  La  reaction  du  lait  et  de  1'humeur  aqueuse  etudiee  par 
la  methode  electrometrique,  C.-R.  Soc.  Biol.,  1905,  vol.  59,  pp.  51-53. 

212  Michaelis,  L.,  and  Mendelssohn,  A.,  Die  Wirkungsbedingungen 
des  Labferments,  Biochem.  Zeitschr.,  1913,  vol.  58,  pp.  315-328. 

D.  MISCELLANEOUS  BODY  FLUIDS  AND  TISSUES. 

213  Allaria,  G.  B.,  Untersuchungen  iiber  Wasserstoff-Ionen-Konzen- 
tration   im   Sauglingsmagen,   Jahr.   f.   Kinderheilk.,   Erganzungsband 
1908,  vol.  67,  pp.  123-142. 

214  Auerbach,  F.,  and  Pick,  H.,  Die  Alkalitat  von  Pankreassaft  und 
Darmsaft  lebender  Hunde,  Arbeit,  a.  d.  kais.  Gesundheitsamte,  1913, 
vol.  43,  pp.  155-186. 

215  Bisgaard,  A.,  Untersuchungen  iiber  die  Eiweiss-  und  Stiekstoff- 
verhaltnisse  der  Cerebrospinalfliissigkeit  sowie  iiber  die  Wasserstoff- 
ionenkonzentration   derselben,  Biochem.  Zeitschr.,  1913,  vol.   58,  pp. 
1-64. 


56     University  of  California  Publications  in  Physiology     [VOL.  5 

216  Christiansen,  J.,  Die  Sauerstoffionen-Konzentratiou  iin  Magen- 
inhalt,  Deut.  Arch.  f.  klin.  Med.,  1911,  vol.  102,  pp.  103-116. 

21?  Christiansen,  J.,  Bestimmung  freier  Salzsaure  im  Mageninhalt, 
Biochem.  Zeitschr.,  1912,  vol.  46,  pp.  24-49. 

218  Davidsohn,  H.,  Beitrag  zum  Chemismus  des  Sauglingsmagens, 
Zeitschr.  f.  Kinderheilk.,  1911,  vol.  2,  pp.  420-428. 

219  Felton,  L.  D.,  Hussey,  R.  G.,  and  Bayne-Jones,  S.,  The  reaction 
of  the  cerebrospinal  fluid,  Arch  Int.  Med.,  1917,  vol.  19,  pp.  1085-1096. 

220  Foa,  C.,  La  reaction  des  liquides  de  1  'organisme  etudiee  par  la 
methode  electrometrique,  C.-E.  Soc.  biol.,  1905,  vol.  58,  pp.  865-866. 

221  Foa,    C.,    La    reaction    de    quelques    liquides    de    1  'organisme 
etudiee  par  la  methode  electrometrique,  C.-R.  Soc.  Biol.,  1905,  vol.  58, 
pp.   1000-1002. 

222  Foa,  C.,  La  reaction  du  sue  gastrique;  etudiee  par  la  methode 
electrometrique,  C.-E.  Soc.  Biol.,  1905,  vol.  59,  pp.  2-4. 

223  Foa,   C.,  La  reazione  dei  liquidi  dell '   organismo   determinata 
col  metodo  elettrometrico    (pile  di  concentrazione),  Arch,   di  Fisiol- 
ogica,  1906,  vol.  3,  pp.  369-415. 

224  Fraenckel,    P.,    Die    Wasserstoffionenconcentration    des    reinen 
Magensaftes  und  ihre   Beziehung  zur  elektrischen  Leitfahigkeit  und 
zur  titrimetrischen  Aciditat,  Zeitschr.  exper.  Path.  u.  Therap.,  1905, 
vol.  1,  pp.  431-438. 

225  Fraenckel,    P.,    Ueber    den    Einfluss    der    Erdalkalien    auf    die 
Eeaction  thierischer   Safte,   Zeitschr.   exper.   Path.   u.    Therap.,   1905, 
vol.  1,  pp.  439-445. 

226  Galeotti,  G.,  Sui  fenomeni  elettrici  del  cuore.     Variazioni  della 
concentrazione    degli   H-ioni    nel    mioplasma    duraute    la    contrazione 
o  nella  morte  del  cuore,  Arch,  di  Fisiologica,  1904,  vol.  1,  pp.  512-530. 

227  Henderson,  L.  J.,   The  theory  of  neutrality  regulation  in  the 
animal  organism,  Am.  Jour.  Physiol.,  1908,  vol.  21,  pp.  427-448. 

228  Henderson,    L.    J.,    Das    Gleichgewicht    zwischen    Baseu    und 
Sauren   im  tierischen   Organismus,   Ergeb.   d.   Physiol.,   1909,   vol.    8, 
pp.  254-325. 

229  Henderson,  L.  J.,  A  critical  study  of  the  process  of  acid  excre- 
tion. Jour.  Biol.  Chem.,  1911,  vol.  9,  pp.  403-424. 

230  Hess,  R.,  Die  Aeiditat  des  Sauglingsmagens,  Zeitschr.  f .  Kinder- 
heilk., 1915,  vol.  12,  pp.  409-439. 

231  Hober,  E.,  Die  Beteiligung  von  Wasserstoff-  und  Hydroxylionen 
bei  physiologischen  Vorgangen,  Zeitschr.  Electrochem.,  1910,  vol.  16, 
pp.  681-686. 

232  Howe,  P.  E.,  and  Hawk,  P.  B.,  Hydrogen  ion  concentration  of 
feces,  Jour.  Biol.  Chem.,  1912,  vol.  11,  pp.  129-140. 

233  Hurwitz,   S.  H.,  and  Tranter,  C.  L.,  On  the  reaction  of  the 
cerebrospinal  fluid,  Arch.  Int.  Med.,  1916,  vol.  17,  pp.  828-839. 

234  Lob,  W.,  and  Higuchi,  S.,  Die  Wasserstoff-  und  Hydroxylionen- 
konzentrationen   des   Placentar-   und   Eetroplacentarserums,   Biochem. 
Zeitschr.,  1910,  vol.  24,  pp.  92-107. 

235  Long,  J.  H.,  and  Fenger,  F.,  On  the  reaction  of  the  pancreas, 
Jour.  Am.  Chem.  Soc.,  1915,  vol.  37,  pp.  2213-2219. 

236  Long,  J.  H.,  and  Fenger,  F.,  On  the  reaction  of  the  pancreas 
and  other  organs,  Jour.  Am.  Chem.  Soc.,  1916,  vol.  38,  pp.  1115-1128. 


1919]     Schmidt-Hoagland:  Table  of  PH,  H+  and  OH-  Values    57 

237  McClendon,  J.  F.,  Acidity  curves  in  the  stomachs  and  duodenum 
of  adults  and  infants,  plotted  with  the  aid  of  improved  methods  of 
measuring    hydrogen    ion    concentration,    Am.    Jour.    Physiol.,    1915, 
vol.  38,  pp.  191-199. 

238  McClendon,  J.  F.,  Shedlov,  A.,  and  Thomson,  W.,  The  hydro- 
gen ion  concentration  of  the  ileum  content,  Jour.  Biol.  Chem.,  1917, 
vol.  31,  pp.  269-270. 

239  McClendon,  J.  F.,  Shedlov.,  A.,  and  Karpman,  B.,  The  hydro- 
gen ion  concentration  of  the  contents  of  the  small  intestine,  Jour. 
Biol.  Chem.,  .1918,  vol.  34,  pp.  1-3. 

240  Menten,  M.  L.,  Acidity  of  undiluted  normal  gastric  juice  from 
a  case  of  human  gastric  fistula,  Jour.  Biol.  Chem.,  1915,  vol.  22,  pp. 
341-343. 

241  Michaelis,    L.,    and    Davidsohn,    H.,    Die    Bedeutung    und    die 
Messung   der   Magensaftaciditat,   Zeitschr.    exper.    Path.    u.    Therap., 
1910,  vol.   8,  pp.   398-413. 

242  Michaelis,   L.,    and   Kramsztyk,    A.,   Die   Wasserstoffionenkon- 
zentration   der   Gewebssafte,   Biochem.    Zeitschr.,    1914,    vol.    62,    pp. 
180-486. 

243  Okada,  S.,  On  the  reaction  of  bile,  Jour.  Physiol.,   1915,  vol. 
50,  pp.  114-118. 

244  Quagliariello,   G.,   Sulla   reazione    chimica    della    bile,    Atti    d. 
Eeale  Acead.  d.  Lincei,  Eome,  1911,  vol.  20,  pp.  302-305. 

245  Eosemann,  B.,  Physiologic  der  Verdauung.     VII,  H-ionen  Kon- 
zentration    des    Magensaftes.,   Arch.    f.    d.    ges.    Physiol.,    1917,    vol. 
169,  pp.  188-200,  quoted  from  Physiol.  Abst.,  1918,  vol.  2,  p.  604. 

246  Salge,  B.,   Salzsaure  im   Sauglingsmagen,  Zeitschr.   f.   Kinder- 
heilk.,  1912,  vol.  4,  pp.  171-173. 

247  Tangl,  F.,  Untersuchungen  iiber  die  Hydrogenionenkonzentra- 
tion  im  Inhalte  des  niichternen  menschlichen  Magens,  Arch.  f.  d.  ges. 
Physiol.,  1906,  vol.  115,  pp.  64-71. 

E.  PEOTEINS. 

248  Bugarszky,   S.,  and  Liebermann,   L.,   Ueber   das   Bindungsver- 
mb'gen   eiweissartiger   Korper   fur    Salzsaure,    Natriumhydroxyd    und 
Kochsalz,  Arch.  f.  d.  ges.  Physiol.,  1898,  vol.  72,  pp.  51-74. 

249  Chick,  H.,  and  Martin,  C.  J.,  On  the  "heat  coagulation"  of 
proteins,  Jour.   Physiol.,   1910,   vol.   40,   pp.   404-430;    1911,   vol.   43, 
pp.  1-27. 

250  Chick,  H.,  and  Martin,  C.  J.,  Die  Hitzekoagulation  der  Eiweiss- 
kb'rper,  Kolloid.  chem.  Beihefte,  1913,  vol.  5,  pp.  49-140. 

251  Henderson,  L.  J.,  Palmer,  W.  W.,  and  Newburgh,  L.  H.,  The 
swelling  of   colloids   and   hydrogen   ion   concentration,   Jour.   Pharm. 
and  Exper.  Therap.,  1914,  vol.  5,  pp.  449-467. 

252  Manabe,  K.,  and  Matula,  J.,  Elektrochemische  Untersuchungen 
am  Saureeiweiss,  Biochem.  Zeitschr.,  1913,  vol.  52,  pp.  369-408. 

253  Michaelis,  L.,  Die  elektrische  Ladung  des  Serumalbumins  und 
der  Fermente,  Biochem.  Zeitschr.,  1909,  vol.  19,  pp.  181-185. 

254  Michaelis,  L.,  Ueber  die  Dissoziation  der  amphoteren  Elektro- 
lyte,  Biochem.  Zeitschr.,  1911,  vol.  33,  pp.  182-189. 

255  Michaelis,  L.,   Zur   Theorie   des   isoelektrischen   Punktes.      Ill, 
Das  Wesen  der  Eiweissartigen  kolloidalen  Losungen,  Biochem.  Zeit- 
schr. 1912,  vol.  47,  pp.  250-259. 


58     University  of  California  Publications  in  Physiology     [VOL.  5 

256  Michaelis,  L.,  and  Davidsohn,  H.,  Der  isoelektrische  Punkt  des 
gemeinen  und  des  denaturierten   Serumalbumins,  Bioehem.   Zeitschr., 

1911,  vol.  33,  pp.  456-473. 

257  Michaelis,  L.,  and  Davidsohn,  H.,  Ueber  das  Flockungsoptimum 
von  Kolloidgemischen,  Bioehem.  Zeitschr.,  1912,  vol.  39,  pp.  496-506. 

258  Michaelis,  L.,  and  Davidsohn,  H.,  Ueber  die  Kataphorese  des 
Oxyhamoglobins,  Bioehem.  Zeitschr.,  1912,  vol.  41,  pp.  102-110. 

259  Michaelis,  L.,  and  Davidsohn,  H.,  Die  Abhangigkeit  spezifischer 
Fallungsreaktionen  von  der  Wasserstoffionenkonzentration,  Bioehem. 
Zeitschr.,  1912,  vol.  47,  pp.  59-72. 

260  Michaelis,  L.,  and  Davidsohn,  H.,  Zur  Theorie  des  isoelektrischen 
Punktes,  Bioehem.  Zeitschr.,  1910,  vol.  30,  pp.  143-150. 

261  Michaelis,  L.,  and  Davidsohn,  H.,  Weiterer  Beitrag  zur  Frage 
nach   der   Wirkung   der    Wasserstoffionenkonzentration    auf    Kolloid- 
gemische,  Bioehem.  Zeitschr.,   1913,  vol.   54,  pp.   323-329. 

262  Michaelis,   L.,  and   Grineff,  W.,   Der  isoelektrische   Punkt   der 
Gelatine,  Bioehem.  Zeitsehr.,  1912,  vol.  41,  pp.  373-374. 

263  Michaelis,  L.,  and  Mostynski,  B.,  Die  isoelektrische  Konstante 
und    die    relative    Aciditatskonstante    des    Serumalbumins,    Bioehem. 
Zeitschr.,  1910,  vol.  24,  pp.  79-91. 

264  Michaelis,    L.,    and    Mostynski,    B.,    Die    innere    Eeibung    von 
Albuminlosungen,  Bioehem.  Zeitschr.,  1910,  vol.  25,  pp.  401-410. 

265  Michaelis,  L.,  and  Pechstein,  H.,  Der  isoelektrische  Punkt  des 
Caseins,  Bioehem.  Zeitschr.,  1912,  vol.  47,  pp.  260-268. 

266  Miehaelis,  L.,  and  Eona,  P.,  Die  Koagulation  des  denaturierten 
Albumins   als   Funktion    der   Wasserstoffionenkonzentration   und   der 
Salze,  Bioehem  Zeitschr.,  1910,  vol.  27,  pp.  38-52. 

267  Michaelis,  L.,  and  Eona,  P.,  Ueber  die  Fallung  des  Globuline 
im  isoelektrischen  Punkt,  Bioehem.  Zeitschr.,  1910,  vol.  28,  pp.  193- 
199. 

268  Quagliariello,   G.,   Die   Anderung   der   Wasserstoffionenkonzen- 
tration wahrend  der  Hitzkoagulation  der  Proteine,  Bioehem.  Zeitschr., 

1912,  vol.  44,  pp.  157-161. 

2<39  Eoberson,  T.  B.,  On  the  dissociation  of  serum  globulin  at  vary- 
ing hydrogen  ion  concentrations,  Jour.  Phys.  Chem.,  1907,  vol.  11, 
pp.  437-460. 

270  Eobertson,  T.  B.,  The  dissociation  of  potassium  caseinate  in 
solutions   of   varying   alkalinity,   Jour.    Phys.    Chem.,    1910,   vol.    14, 
pp.  528-568. 

271  Eobertson,  T.  B.,  The  dissociation  of  the  salts  of  ovomucoid 
in  solutions   of  varying  alkalinity  and  acidity,  Jour.   Phys.   Chem., 
1910,  vol.  14,  pp.  709-718. 

272  Schmidt,  C.  L.  A.,  Changes  in  the  B>  and  OH~  concentration 
which  take  place  in  the  formation  of  certain  protein  compounds.  Jour. 
Biol.  Chem.,  1916,  vol.  25,  pp.  63-79. 

273  Schmidt,   C.   L.   A.,   Studies   on  the  formation   and   antigenic 
properties  of  certain  compound  proteins,  Univ.   Calif.  Publ.   Path., 
1916,  vol.  2,  pp.  157-204. 

274  Spiro,  K.,  Die  Fallung  von  Kolloiden,  Bioehem.  Zeitschr.,  1913, 
vol.  56,  pp.  11-16. 

275  Sorensen,  S.  P.  L.,  and  Jiirgensen,  E.,  La  concentration  en  ions 
hydrogene  du  milieu  subit-elle  des  modifications  par  suite  de  la  coagu- 
lation?   C.-E.  Lab.,  Carlsberg,  1911,  vol.  10,  pp.  1-51. 


Schmidt-H&agland:  Table  of  PH,  H+  and  OH-  Values     59 

276  Sorensen,  S.  P.  L.,  and  Jiirgensen,  E.,  Wird  die  Wasserstoff- 
ionenkonzentration  der  Losung,  durch  die  Koagulation  geandert,  Bio- 
chem.  Zeitschr.,  1911,  vol.  31,  pp.  397-442. 

277  Ylppo,    A.,    Der    isoelektrische    Punkt    des    Menschen-    Kuh- 
Ziegen-  Hunde-  und  Meerschweinschenmilchcaseins,  Zeitschr.  f.  Kinder- 
heilk.,  1913,  vol.  8,  pp.  224-234. 

F.  ENZYMES. 

278  Adler,  L.,  The  influence  of  the  hydrion  concentration  on  the 
activity  of  malt  diastase,  Biochem.  Zeitschr.,  1916,  vol.  77,  pp.  146- 
167,  quoted  from  Physiol.  Abst.,  1917,  vol.  2,  p.  17. 

279  Ambard,  M.,  and  Foa,  C.,  Les  modifications  de  1  'acidite  d  'un 
melange  sue  gastrique-albumine  au  cours  de  la  digestion,  C.-E.  Soe. 
Biol.,  1915,  vol.  59,  pp.  5-9. 

280  Auerbach,  F.,  and  Pick,  H.,  Bemerkung  zur  Pankreasverdauung, 
Biochem.  Zeitschr.,  1913,  vol.  48,  pp.  425-426. 

281  Compton,    A.,    The    influence    of    the    hydrogen .  concentration 
upon  the  optimum  temperature  of  a  ferment,  Proc.  Koy.  Soc.,  London, 
(B)  1914,  vol.  88,  pp.  408-417. 

282  Van  Dam.,  W.,  Beitrag  zur  Kenntnis  der  Labgerinnung,  Zeit- 
schr. f.  physiol.  Chem.,  1909,  vol.  58,  pp.  295-330. 

283  Davidsohn,  H.,  Die  Pepsinverdauung  im  Sauglingsmagen  unter 
Beriicksichtigung  der  Aciditat,  Zeitschr.  f.  Kinderheilk.,  1912,  vol.  4, 
pp.  208-230. 

284  Davidsohn,  H.,  Beitrag  zum  Studium  der  Magenlipase,  Biochem. 
Zeitschr.,  1912,  vol.  45,  pp.  284-302. 

285  Davidsohn,   H.,   Ueber   die   Abhangigkeit   der   Lipase   von   der 
Wasserstoffionenkonzentration,  Biochem.  Zeitschr.,  1913,  vol.  49,  pp. 
249-277. 

286  Dernby,  K.  G.,  Etude  sur  la  cinetique  d  'une  hydrolyse  enzy- 
matique  de  la  glycylglycocolle,  C.-E.  Lab.,  Carlsberg,  1916,  vol.  11, 
pp.  263-294. 

287  Emslander,   F.,   Die   Wasserstoffionen-Konzentration   im   Biere 
und  bei  dessen  Bereitung,  Kolloid  Zeitschr.,  1913,  vol.  13,  pp.   156- 
169;  1914,  vol.  14,  pp.  44-48. 

288  Hagglund,   E.,   Hefe   und   Garung   in   ihrer   Abhangigkeit  von 
Wasserstoff-  und  Hydroxylionen,  Sammlung  chem.  u.  chem.-tech.  Vor- 
trage,  1914,  vol.  21,  pp.  129-174. 

289  Hagglund,    E,    Ueber    die    garungshemmende    Wirkung    der 
Wasserstoffionen,  Biochem.  Zeitschr.,  1915,  vol.  69,  pp.  181-191. 

290  Leberle,   H.,  and  Liiers,  H.,   Acid   determination   in   beer   by 
electrometrical   methods,   Zeitschr.   ges.   Brau.,  vol.    37,   pp.    177-184, 
quoted  from  Chemical  Abst.,  1914,  vol.  8,  p.  2447. 

291  Liiers,  H.,  Change  of  hydrogen  ion  concentration  during  fer- 
mentation, Zeitschr.  ges.  Brau.,  vol.  37,  pp.  79-82,  quoted  from  Chem- 
ical Abst.,  1914,  vol.  8,  p.  1845. 

292  Michaelis,  L.,  Zur  Theorie  der  elektrolytischen  Dissoziation  der 
Fermente,  Biochem.  Zeitschr.,  1914,  vol.  60,  pp.  91-96. 

293  Michaels,  L.,  and  Davidsohn,  H.,  Die  isoelektrische  Konstante 
des  Pepsins,  Biochem.  Zeitschr.,  1910,  vol.  28,  pp.  1-6. 

29*  Miehaelis,  L.,  and  Davidsohn,  H.,  Trypsin  und  Pankreasnucleo- 
proteid,  Biochem.  Zeitschr.,  1910,  vol.  30,  pp.  481-504. 


60     University  of  California  Publications  in  Physiology     [VOL.  5 

295  Michaelis,  L.,  and  Davidsohn,  H.,  Die  Wirkung  der  Wasserstoff- 
ionen  auf  das  Invertin,  Biochem.  Zeitsehr.,  1911,  vol.  35,  pp.  386-412. 

296  Michaelis,  L.,  and  Davidsohn,  H.,  Die  Abhangigkeit  der  Tryp- 
simvirkung  von  der  Wasserstoffionenkonzentration,  Biochem.  Zeitsehr., 

1911,  vol.  36,  pp.  280-290. 

297  Michaelis,  L.,  and  Mendelssohn,  A.,  Die  Wirkungsbedingungen 
des  Pepsins,  Biochem.  Zeitsehr.,  1914,  vol.  65,  pp.  1-15. 

298  Michaelis,  L.,  and  Menten,  M.  L.,  Die   Kinetik  der  Invertin- 
wirkung,  Biochem.  Zeitsehr.,  1913,  vol.  49,  pp.  333-369. 

299  Michaelis,    L.,    and    Pechstein,    H.,    Untersuchungen    iiber    die 
Katalase  der  Leber,  Biochem.  Zeitsehr.,  1913,  vol.  53,  pp.  320-355. 

soo  Michaelis,  L.,  and  Pechstein,  H.,  Die  Wirkungsbedingungen 
der  Speicheldiastase,  Biochem.  Zeitsehr.,  1914,  vol.  59,  pp.  77-99. 

soi  Michaelis,  L.,  and  Eona,  P.,  Ueber  die  Umlagerung  der 
Glucose  bei  alkalischer  Eeaktion;  ein  Beitrag  zur  Theorie  der  Kata- 
lyse,  Biochem.  Zeitsehr.,  1912,  vol.  47,  pp.  447-461. 

302  Michaelis,  L.,  and  Eona,  P.,  Die  Wirkungsbedingungen  der 
Maltase  aus  Bierhefe  I.  Biochem.  Zeitsehr.,  1913,  vol.  57,  pp.  70-83. 

sos  Morse,  M.,  Hydrogen  ion  concentration  in  autolysis,  Jour. 
Biol.  Chem.,  1916,  vol.  24,  Proc.  Soc.  Biol.  Chem.,  p.  xxvii. 

304  Norris,  E.  V.,  The  hydrolysis  of  glycogen  by  diastatic  enzymes. 
Comparison  of  preparations  of  glycogen  from  different  sources, 
Biochem.  Jour.,  1913,  vol.  7,  pp.  26-42. 

sos  Palitzseh,  S.,  and  Walbum,  L.  E.,  Sur  la  concentration  optimale 
des  ions  hydrogene  pour  la  premiere  phase  de  la  decomposition 
trypsique  de  la  gelatine  (Liquefaction  de  la  gelatine),  C.-E.  Lab., 
Carlsberg,  1912,  vol.  9,  pp.  200-236. 

soe  Palitzseh,  S.,  and  Walbum,  L.  E.,  Ueber  die  optimale  Wasser- 
stoffionenkonzentration  bei  der  tryptischen  Gelatineverfliissigung, 
Biochem.  Zeitsehr.,  1912,  vol.  47,  pp.  1-35. 

SOT  Eeed,  G.  B.,  The  relation  of  oxidase  reactions  to  changes  in 
hydrogen  ion  concentration,  Jour.  Biol.  Chem.,  1916,  vol.  27,  pp. 
299-302. 

sos  Eeed,  G.  B.,  Measurement  of  oxidation  potential,  and  its  sig- 
nificance in  the  study  of  oxidases,  Bot.  Gaz.,  1917,  vol.  61,  pp.  523- 
527. 

309  Einger,  W.  E.,  and  Van  Tright,  H.,  Einfluss  der  Eeaktion  auf 
die   Ptyalinwirkung,   Zeitsehr.   f.   physiol.    Chem.,   1912,   vol.    82,   pp. 
484-501. 

310  Eobertson,  T.  B.,  and  Schmidt,  C.  L.  A.,  On  the  part  played 
by  the   alkali  in   the  hydrolysis   of  proteins  by  trypsin,  Jour.   Biol. 
Chem.,  1908,  vol.  5,  pp.  31-48. 

311  Eohonyi,  H.,  Die  Veranderung  der  Wasserstoffionenkonzentra- 
tion    der    Pepsinwirkung    und    das    Saurebindungsvermogen    einiger 
hydrolytischer   Spaltungsprodukte   des   Eiweisses,   Biochem.   Zeitsehr., 

1912,  vol.  44,  pp.  165-179. 

312  Eona,  P.,  Zur  Kenntnis  der  Esterspaltung  im  Blute,  Biochem. 
Zeitsehr.,  1911,  vol.  33,  pp.  413-422. 

sis  Eona,  P.,  and  Arnheim,  F.,  Beitrag  zur  Kenntnis  des  Erepsins, 
Biochem.  Zeitsehr.,  1913,  vol.  57,  pp.  84-94. 

si*  Eona,  P.,  and  Bien,  Z.,  Zur  Kenntnis  der  Esterase  des  Blutes, 
Biochem.  Zeitsehr.,  1914,  vol.  59,  pp.  100-112. 


Schmidt-Hoagland:  Table  of  PH,  H+  and  OH~  Values     61 

sis  Rona,  P.,  and  Bien,  Z.,  Vergleichende  Untersuchungen  iiber 
Pankreaslipase  und  Blutesterase,  Biochem.  Zeitschr.,  1914,  vol.  64, 
pp.  13-29. 

sis  Rona,  P.,  and  Michaelis,  L.,  Ueber  Ester-  und  Fettspaltung  im 
Blute  und  ini  Serum,  Biochem.  Zeitschr.,  1911,  vol.  31,  pp.  345-354. 

SIT  Rona,  P.,  and  Michaelis,  L.,  Die  Wirkungsbedingungen  der 
Maltase  aus  Bierhefe.  II,  Die  Wirkung  der  Maltase  auf  a  Methyl- 
glucosid  und  die  Affinitatsgrbsse  des  Ferments,  Biochem.  Zeitschr., 
1913,  vol.  58,  pp.  148-157. 

sis  Rona,  P.,  and  Wilenko,  G.  G.,  Beitrage  zur  Frage  der  Glykolyse 
IV,  Biochem.  Zeitschr.,  1914,  vol.  62,  pp.  1-10. 

319  Sorensen,  S.  P.  L.,  Enzymstudien.     II,  Ueber  die  Messung  und 
die  Bedeutung  der  Wasserstoffionenkonzentration  bei   enzymatischen 
Prozessen,  Biochem.  Zeitschr.,  1909,  vol.  21,  pp.  131-304. 

320  Sorensen,   S.   P.   L.,   Erganzung  zu   der  Abhandlung:    Enzym- 
studien.    II,  Ueber  die  Messung  und  die  Bedeutung  der  Wasserstoff- 
ionenkonzentration bei  enzymatischen  Prozessen,   Biochem.   Zeitschr., 

1909,  vol.  22,  pp.  352-356. 

321  Sorensen,  S.  P.  L.,  Etudes  enzymatiques.     II,  Sur  la  mesure  et 
1 'importance  de  la  concentration  des  ions  hydrogene  dans  les  reactions 
enzymatiques.     C.-R.  Lab.,  Carlsberg,  1909,  vol.  8,  pp.  1-168,  396-401. 

322  Van  Slyke,  D.  D.,  and  Zacharias,  G.,  The  effect  of  hydrogen  ion 
concentration   and   of   inhibiting   substances    on    urease,    Jour.    Biol. 
Chem.,  1914,  vol.  19,  pp.  181-210. 

G.  SEA  WATER. 

323  Haas,  A.  R.  C.,  The  effect  of  the  addition  of  alkali  to  sea  water 
upon  the  hydrogen  ion  concentration,  Jour.  Biol.   Chem.,   1916,  vol. 
26,  pp.  515-517. 

324  Henderson,  L.  J.,  and  Cohn,  E.  J.,  Equilibrium  between  acids 
and  bases  in  sea  water,  Proc.  Nat.  Acad.  Sci.,  1916,  vol.  2,  pp.  618- 
622. 

325  McClendon,  J.  F.,  New  buffer  mixtures,  standard  tubes,  and 
colorimeter  for   determining  the   hydrogen   ion   concentration   of   sea 
water,  Jour.  Biol.  Chem.,  1916,  vol.   28,  Proc.   Soc.  Biol.  Chem.,  pp. 
xxx-xxxi. 

326  Palitzsch,  S.,  Ueber  die  Messung  und  die  Grb'sse  der  Wasser- 
stoffionenkonzentration   des    Meerwassers,    Biochem.    Zeitschr.,    1911, 
vol.  37,  pp.  116-130. 

327  Palitzsch,  S.,  Sur  le  mesurage,  et  la  grandeur  de  la  concentra- 
tion en  ions  hydrogene  de  1'eau  salee,  C.-R.  Lab.,  Carlsberg,  1911, 
vol.  10,  pp.  85-98. 

328  Sorensen,  S.  P.  L.,  and  Palitzsch,  S.,  Sur  "1'erreur  de  sel" 
dans  la  mesure  colorime'trique  de  la  concentration  des  ions  hydrogene 
de  1'eau  de  mer,  C.-R.  Lab.,  Carlsberg,  1911,  vol.  10,  pp.  252-258. 

329  Sorensen,  S.  P.  L.,  and  Palitzsch,  S.,   Sur  le  mesurage  de  la 
concentration  en  ions  hydrogene  de  1'eau  de  mer,  C.-R.  Lab.,  Carls- 
berg, 1910,  vol.  9,  pp.  8-37. 

330  Sorensen,  S.  P.  L.,  and  Palitzsch,  S.,  Ueber  die  Messung  der 
Wasserstoffionenkonzentration   des  Meerswassers,   Biochem.   Zeitschr., 

1910,  vol.  24,  pp.  387-415. 


62     University  of  California  Piiblioations  in  Physiology     [VOL.  5 
III.  BACTERIOLOGICAL. 

331  Ayers,    S.    H.,    Hydrogen-ion    concentrations    in    cultures    of 
streptococci,  Jour.  Bact.,  1916,  vol.  1,  pp.  84-85. 

332  Beniasch,  M.,  Die  Saureagglutination  der  Bakterien,  Zeitschr. 
f.  Immunitatsfrsch.  u.  exper.  Therap.,  1912,  vol.  12,  pp.  268-315. 

333  Clark,   W.   M.,   The    influence   of   hydrogen-ion   concentrations 
upon  the  physiological  activities  of  Bacillus  coli,  Science,  n.s.,  1915, 
vol.  41,  p.  624.    * 

33*  Clark,  W.  M.,  The  final  hydrogen  ion  concentrations  of  cultures 
of  Bacillus  coli,  Jour.  Biol.  Chem.,  1915,  vol.  22,  pp.  87-98. 

335  Clark,  W.  M.,  The  "reaction"  of  bacteriologic  culture  media, 
Jour.  Infec.  Dis.,  1915,  vol.  17,  pp.  109-136. 

sse  Clark,  W.  M.,  and  Lubs,  H.  A.,  The  differentiation  of  bacteria 
of  the  colon-aerogenes  family  by  the  use  of  indicators,  Jour.  Infec. 
Dis.,  1915,  vol.  17,  pp.  160-173. 

337  Clark,  W.  M.,  and  Lubs,  H.  A.,  The  colorimetric  determination 
of  hydrogen  ion  concentration  and  its  applications  in  bacteriology, 
Jour.  Bact.,  1917,  vol.  2,  pp.  1-34,  109-136,  191-236. 

338  Gillespie,  L.  J.,  The  acid  agglutination  of  pneumococci,  Jour. 
Exper.  Med.,  1914,  vol.  19,  pp.  28-37. 

339  Grote,  L.  E.,  Ueber  die  praktische  Verwertbarkeit  der  Saure- 
agglutination   nach    Michaelis,    Centrbl.    Bakt.    Orig.,    1913,    vol.    69, 
pp.  98-104. 

340  Heimann,  W.,  Die  "Saureagglutination"  innerhalb  der  Typhus- 
Paratyphusgruppe,  insbesondere  sogenannter  Paratyphus-  C-  Baccillen, 
Zeitschr.  f.  Immunitatsfrsch.,  1912,  vol.  16,  pp.  127-140. 

341  Henderson,  L.   J.,   and   Webster,   H.   B.,    The   preservation   of 
neutrality  in  culture  media  with  the  aid  of  phosphates,  Jour.  Med. 
Ees.,  1907,  vol.  16,  pp.  1-5. 

342  Homer,  A.,  The  reaction  of  sera  as  a  factor  in  the  successful 
concentration   of   antitoxic   sera  by   the   methods   at   present   in   use, 
Biochem.  Jour.,  1917,  vol.  11,  pp.  21-39. 

343  Hurwitz,  S.  H.,  Meyer,  K.  F.,  and  Ostenberg,  Z.,  On  a  colori- 
metric  method    of    adjusting    bacteriological    culture    media    to    any 
optimum   hydrogen   ion   concentration,   Proe.    Soc.    Exper.    Biol.    and 
Med.,  1915,  vol.  13,  pp.  24-26. 

344  Hurwitz,  S.  H.,  Meyer,  K.  F.,  and  Ostenberg,  Z.,  A  colorimetric 
method  for  the  determination  of  the  hydrogen  ion  concentration  of 
biological  fluids,  with  special  reference  to  the  adjustment  of  bacterio- 
logical culture  media,  Johns  Hopkins  Hosp.  Bull.,  1916,  27,  pp.  16-24. 

345  Itano,  A.,  The  relation  of  hydrogen  ion  concentration  of  media 
to  the  proteolytic  activity  of  Bacillus  subtilis,  Mass.  Agr.  Exp.  Sta. 
1916,  Bull.  no.  167,  pp.  139-177. 

346  Lindenschatt,  S.  M.,  Ueber  den  Einfluss  der  OH~  and  H+  ionen 
auf    die    Komplementablenkung    und    das    differente    Verhalten    ver- 
schieden  hoch  erhitzter  Sera  bei  der  Komplementfixierung.     Dissert. 
Heidelberg,  1913,  pp.  1-39,  quoted  from  Zentrbl.  f.  Biochem.  u.  Bio- 
physik.,  1914,  vol.  16,  p.  504. 

347  Markl,    J.    G.,    Ueber    Saureagglutination    von    Pestbacillen, 
Centrbl.  Bakt.  Orig.,  1915,  vol.  77,  pp.  102-108. 

348  Meyer,   K.,   Zur   Kenntniss   der   Bakterienproteasen,    Biochem. 
Zeitsch.,  1911,  vol.  32,  pp.  274-279. 


Schmidt-Hoagland:  Table  of  PH,  H+  and  OH"  Values     63 

349  Michaelis,  L.,  Die  Saureagglutination  der  Bakterien,  insbeson- 
dere  der  Typhusbazillen,  Deut.  med.  Woeh.,  1911,  vol.  37,  pp.  969-971. 

sso  Michaelis,  L.,  and  Marcora,  F.,  Die  Saureproduktivitat  des 
Bacterium  coli,  Zeitschr.  f.  Immunitatsfrseh.  u.  exper.  Therap.,  1912, 
vol.  14,  pp.  170-173. 

351  Miehaelis,  L.,  and  Skwirsky,  P.,  Der  Einfluss  der  Eeaktion  auf 
die    spezifische    Hamolyse,    Zeitschr.    f.    Immunitatsfrsch.    u.    exper. 
Therap,.  1910,  vol.  4,  pp.  357-374,  629-635.      - 

352  Michaelis,  L.,  and  Takahashi,  D.,  Die  isoelektrischen  Konstan- 
ten  der  Blutkorperchenbestandteile  und  ihre  Beziehungen  zur  Saure- 
hamolyse,  Biochem.  Zeitschr.,  1910,  vol.  29,  pp.  439-452. 

sss  Poppe,  Dr.,  Die  Saureagglutination  der  Bakterien  der  Para- 
typhusgruppe,  Zeitschr.  f.  Immunitatsfrsch.  u.  exper.  Therap.,  1912, 
vol.  13,  pp.  185-191. 

354  Walbum,   L.   E.,   Die   Bedeutung   der   Wasserstoffionenkonzen- 
tration  fiir  die  Hamolyse,  Biochem.  Zeitschr.,  1914,  vol.  63,  pp.  221- 
268. 

355  Waterman,  H.  J.,  Ueber  einige  Faktoren  welche  die  Entwicke- 
lung  von  Penicillium  glaucum  beeinflussen.    Beitrag  zur  Kenntnis  der 
Antiseptica  und  der  Narkose,  Ceutrbl.  f.  Bakt.,  2.  Abt.,  1915,  vol.  42, 
pp.  639-688. 

IV.  SOIL  AND  PLANT. 

sse  Conner,  S.  D.,  Acid  soils  and  effect  of  acid  phosphate  and 
other  fertilizers  upon  them,  Jour.  Ind.  Eng.  Chem.,  1916,  vol.  8, 
pp.  35-40. 

SST  Fischer,  G.,  Die  Sauren  und  Kolloide  des  Humus,  Kiihn  Arch., 
1914,  vol.  4,  pp.  1-36. 

358  Gillespie,  L.  J.,  The  reaction  of  soil  and  measurements  of 
hydrogen-ion  concentration,  Jour.  Wash.  Acad.  Sci.,  1916,  vol.  6,  pp. 
7-16. 

sso  Gillespie,  L.  J.,  and  Hurst,  L.  A.,  Hydrogen  ion  concentration 
measurements  of  soils  of  two  types:  caribou  loam  and  washburn 
loam,  Soil  Science,  1917,  vol.  4,  pp.  313-319. 

sso  Haas,  A.  E.  C.,  The  acidity  of  plant  cells  as  shown  by  natural 
indicators,  Jour.  Biol.  Chem.,  1916,  vol.  27,  pp.  233-241. 

ssi  Haas,  A.  B.  C.,  Eeaction  of  plant  protoplasm,  Bot.  Gaz.,  1917, 
vol.  63,  pp.  225-228. 

362  Haas,  A.  E.  C.,  The  excretion  of  acid  by  roots,  Proc.  Nat.  Acad. 
'  Sci.,  1916,  vol.  2,  pp.  561-566. 

ses  Haas,  A.  E.  C.,  Anesthesia  and  respiration,  Science,  n.s.,  1917, 
vol.  46,  pp.  462-464. 

364  Hoagland,  D.  E.,  The  effect  of  hydrogen  and  hydroxyl  ion 
concentration  on  the  growth  of  barley  seedlings,  Soil  Science,  1917, 
vol.  3,  pp.  547-560. 

ses  Hoagland,  D.  E.,  and  Sharp,  L.  T.,  Eelation  of  carbon  dioxide 
to  soil  reaction  as  measured  by  the  hydrogen  electrode,  Jour.  Agr. 
Ees.,  1918,  vol.  12,  pp.  139-148. 

see  Miyake,  K.,  Toxic  action  of  soluble  aluminum  salts  upon  the 
growth  of  the  rice  plant,  Jour.  Biol.  Chem.,  1916,  vol.  25,  pp.  23-28. 

367  Pantanelli,  E.,  Ueber  lonenauf  nahme,  Jahrb.  wiss.  Bot., 
Pringsheim,  1915,  vol.  56,  pp.  689-733. 


64     University  of  California  Publications  in  Physiology     [VOL.  5 

ses  Plummer,  J.  K.,  Studies  in  soil  reaction  as  indicated  by  the 
hydrogen  electrode,  Jour.  Agric.  Res.,  1918,  vol.  12,  pp.  19-31. 

369  Saidel,    T.,    Quantitative    Untersuchungen    iiber    die    Eeaktion 
wasseriger    Bodenausziige,    Bull.    Sect.    Sci.    Acad.    Roumaine,    1913, 
Ann.  2,  pp.  38-44. 

370  Sharp,  L.  T.,  and  Hoagland,  D.  R.,  Acidity  and  adsorption  in 
soils  as  measured  by  the  hydrogen  electrode,  Jour.  Agric.  Res.,  1916, 
vol.  7,  pp.  123-145. 

371  Wagner,  R.   J.,  Wasserstoffionenkonzentration   und  natiirliche 
Immunitat   der   Pflanzen,   Centrbl.   f.   Bakt.,   2.   Abt.,   1916,   vol.   44, 
pp.  708-719. 

V.  MISCELLANEOUS. 

372  Auerbach,  F.,  and  Pick,  H.,  Die  Alkalitat  wasseriger  Losungen 
kohlensaurer  Salze,  Arbeit,  a.  d.  kais.  Gesundheitsamte,  1912,  vol.  38, 
pp.  243-274. 

373  Bethe,  A.,  Die  Bedeutung  der  Elektrolyten  fiir  die  rhythmisehen 
Bewegungen    der    Medusen,    Angriffspunkt    der    Salze,    Einfluss    der 
Anionen  und  Wirkung  der  OH~  und  H+  lonen,  Arch,  f .  d.  ges.  Physiol., 
1909,  vol.  127,  pp.  219-273. 

374  Bjerrum,   N.,    Studien    iiber    chromichlorid,    Zeitschr.    f .    phys. 
Chem.,  1907,  vol.  59,  pp.  336-383. 

375  Bjerrum,  N.,  Studien  iiber  chromichlorid.     Ill,  Hydroxoaquo- 
chromichloride,  Zeitschr.  f.  phys.  Chem.,  1910,  vol.  73,  pp.  724-759. 

376  Brode,  J.,  and  Lange,  W.,  Beitrage  zur  Chemie  des  Essigs  mit 
besonderer  Beriicksichtigung   seiner  Untersuchungsvcrfahren,   Arbeit. 
a.  d.  kais.  Gesundheitsamte,  1909,  vol.  30,  pp.  1-54. 

377  Cohn,  E.  J.,  Relation  between  the  hydrogen-ion  concentration 
of  sperm  suspensions  and  their  fertilizing  power,  Anat.  Rec.,  1917, 
vol.  11,  p.  530. 

378  Dale,  D.,  and  Thacker,  C.  R.  A,,  Hydrogen  ion  concentrations 
limiting  automaticity  in  different  regions  of  the  frog's  heart,  Jour. 
Physiol.,  1914,  vol.  47,  pp.  493-508. 

379  Hildebrand,  J.  H.,  and  Bowers,  W.  G.,  A  study  of  the  action 
of  alkali  on  certain  zinc  salts  by  means  of  the  hydrogen  electrode, 
Jour.  Am.  Chem.  Soe.,  1916,  vol.  38,  pp.  785-788. 

sso  Hildebrand,  J.  H.,  and  Harned,  H.  S.,  The  rapid  determina- 
tion of  magnesia  in  limestone  by  means  of  the  hydrogen  electrode, 
8th  Intern.  Cong.  Appl.  Chem.,  1912,  vol.  1,  pp.  217-225. 

ssi  Jessen-Hansen,  H.,  Influence  de  la  concentration  en  ions  hydro- 
gene  sur  la  valeur  boulangere  de  la  farine,  C.-R.  Lab.,  Carlsberg., 
1911,  vol.  10,  pp.  170-206. 

382  Loeb,  J.,  Ueber  die  Ursachen  der  Giftigkeit  einer  reinen  Chlor- 
natriumlosung  und  ihrer  Entgiftung  durch  K  und  Ca,  Biochem. 
Zeitschr.,  1906,  vol.  2,  pp.  81-110. 

sss  Loeb,  J.,  and  Wasteneys,  H.,  Die  Beeinfliissung  der  Entwicke- 
lung  und  der  Oxydationsvorgange  im  Seeigelei  (Arbacia)  durch 
Basen,  Biochem.  Zeitschr.,  1911,  vol.  37,  pp.  410-423. 

384  Michaelis,  L.,  Die  Saure-  Dissoziationskonstanten  der  Alkohole 
und  Zucker,  insbeesondere  der  Methyl-glucoside,  Ber.  d.  deut.  chem. 
Ges.,  1913,  vol.  46,  pp.  3683-3693. 


1919]     Schmidt-Hoagland:  Table  of  PH,  H+  and  OH-  Values     65 

sss  Michaelis,  L.,  and  Eona,  P.,  Die  Alkaliempfindlichkeit  des 
Traubenzuckers,  Biochem.  Zeitschr.,  1910,  vol.  23,  pp.  364-369. 

386  Paul,  T.,  Der  Sauregrad  des  Weines,  Zeitschr.  f .  Eleetroehem., 

1915,  vol.  21,  pp.  80-89. 

SST  Sand,  H.  J.  S.,  and  Law,  D.  J.,  The  employment  of  the  electro- 
metric  method  for  the  estimation  of  the  acidity  of  tan  liquors,  Jour. 
Soc.  Chem.  Ind.,  1911,  vol.  30,  pp.  3-5. 

388  Szili,  A.,  Experimentelle   Untersuchungen  iiber   Saureintoxika- 
tion,  Arch.  f.  d.  ges.  Physiol.,  1906,  vol.  115,  pp.  82-105. 

389  Szili,   A.,   Weitere   Untersuchungen   iiber   Vergiftung   mit   an- 
organischen  und  organischen  Sauren,  Arch.  f.  d.  ges.  Physiol.,  1909, 
vol.  130,  pp.  134-155. 

390  Wahl,  E.,  New  scientific  conceptions  and  their  application  to 
quality  and  methods  of   preparing  beer,   Am.   Brewers'   Eev.,   1915, 
vol.  29,  pp.  271-274,  365-368,  557-559,  quoted  from  Chemical  Abst., 

1916,  vol.  10,  p.  1398. 

391  Walker,   J.,   and   Kay,   S.   A.,   The   acidity   and   alkalinity   of 
natural  waters,  Jour.  Soc.  Chem.  Ind.,  1912,  vol.  31,  pp.  1013-1016. 

392  Wood,  J.  T.,  Sand,  H.  J.  S.,  and  Law,  D.  J.,  The  employment 
of  the  electrometric  method  for  the  estimation  of  the  acidity  of  tan 
liquors,  Jour.  Soc.  Chem.  Ind.,  1911,  vol.  30,  pp.  872-877. 

VI.  INDICATORS. 

393  Acree,  S.  F.,  On  the  theory  of  indicators  and  the  reactions  of 
phthaleins  and  their  salts,  Am.  Chem.  Jour.,  1908,  vol.  39,  pp.  528- 
544. 

394  Acree,  S.  F.,  and  Slagle,  E.  A.,  On  the  theory  of  indicators 
and  the  reactions  of  phthaleins  and  their  salts,  Am.  Chem.  Jour.,  1909, 
vol.  42,  pp.  115-147. 

395  Bogert,  M.  T.,  and  Scatchard,  G.,  Eesearches  on  quinazolines 
xxxiii.    A  new  and  sensitive  indicator  for  acidimetry  and  alkalimetry, 
and   for  the   determination   of  hydrogen  ion  concentrations  between 
the  limits  of  6  and  8  on  the  Sorensen  scale,  Jour.  Am.  Chem.   Soc., 
1916,  vol.  38,  pp.  1606-1615. 

396  Crozier,  W.  J.,  Some  indicators  from  animal  tissues,  Jour.  Biol. 
Chem.,  1916,  vol.  24,  pp.  443-445. 

397  Fels,   B.,   Studien   iiber   die   Indikatoren   der   Acidimetrie   und 
Alkalimetrie  II,  Zeitschr.  f.  Eleetroehem.,  1904,  vol.  10,  pp.  208-214. 

398  Friedenthal,  H.,  Die  Bestimmung  der  Eeaktion  einer  Fliissig- 
keit  mit  Hilfe  von  Indikatoren,  Zeitschr.  f.  Eleetroehem.,  1904,  vol. 
10,  pp.  113-119. 

399  Harvey,  E.  N.,  A  criticism  of  the  indicator  method  of  deter- 
mining cell  permeability  for  alkalies,  Am.  Jour.  Physiol.,  1913,  vol. 
31,  pp.  335-342. 

400  Henderson,  L.   J.,  and  Forbes,  A.,   On  the  estimation  of  the 
intensity   of   acidity   and   alkalinity  with   dinitrohydroquinone,   Jour. 
Am.  Chem.  Soc.,  1910,  vol.  32,  pp.  687-689. 

401  Hottinger,    E.,    Ueber    ' '  Lackmosol, ' '    den    empfindlichen    Be- 
standtheil   des   Indicators   Lackmoid.   Darstellung  und   einige  Eigen- 
schaften,  Biochem.  Zeitschr.,   1914,  vol.   65,  pp.  177-188. 

402  Kelly,    T.    H.,    Hydrogen-ion   acidity,   Jour.    Lab.    Clin.    Med., 
1915,  vol.  1,  pp.  194-196. 


66     University  of  California  Publications  in  Physiology     [VOL.  5 

403  Lubs,  H.  A.,  and  Acree,  S.  F.,  On  the  sulf  onphthalein  series  of 
indicators  and  the  quinone-phenolate  theory,  Jour.  Am.  Chem.   Soc., 
1916,  vol.  38,  pp.  2772-2784. 

404  Lubs,  H.  A.,  and  Clark,  W.  M.,  On  some  new  indicators  for 
the  colorimetrie   determination   of  hydrogen-ion   concentration,   Jour. 
Wash.  Acad.  Sci.,  1915,  vol.  5,  pp.  609-617. 

405  Lubs,   H.   A.,   and   Clark,   W.   M.,   A   note    on   the    sulphone- 
phthaleins  as  indicators  for  the  colorimetrie  determination  of  hydro- 
gen-ion concentration,  Jour.  Wash.  Acad.  Sci.,  1916,  vol.  6,  pp.  481- 
489. 

406  Micfiaelis,  L.,  and  Bona,  P.,  Zur  Frage  der  Bestimmung  der  H~ 
lonenkonzentration  durch  Indikatoren,  Zeitschr.  f.  Electrochem.,  1908, 
vol.  14,  pp.  251-253. 

407  Michaelis,  L.,  and  Kona,  P.,  Der  Einfluss  der  Neutralsalze  auf 
die  Indicatoren,  Biochem.  Zeitschr.,  1909,  vol.  23,  pp.  61-67. 

408  Noyes,  A.  A.,  Quantitative  application  of  the  theory  of  indi- 
cators to  volumetric  analysis,  Jour.  Am.  Chem.  Soc.,  1910,  vol.  32, 
pp.  815-861. 

409  Palitzsch,  S.,  Sur  1  'emploi  du  rouge  de  methyle  au  mesurage 
colorime'trique   de  la   concentration   en  ions   hydrogene,   C.-E.   Lab., 
Carlsberg,  1911,  vol.  10,  pp.  162-169. 

410  Palitzsch,   S.,   Ueber   die   Verwendung  von   Methylrot   bei   der 
colorimetrischen  Messung  der  Wasserstoffionenkonzentration,  Biochem. 
Zeitschr.,   1911,  vol.   37,  pp.   131-138. 

411  Eosenstein,  L.,  The  ionization  constant  of  phenolphthalein  and 
the  effect  upon  it  of  neutral  salts,  Jour.  Am.  Chem.  Soc.,  1912,  vol. 
34,  pp.  1117-1128. 

412  Salessky,  W.,  Ueber  Indikatoren  der  Acidimetrie  und  Alkali- 
metrie  I,  Zeitschr.  f.  Electrochem.,  1904,  vol.  10,  pp.  204-208. 

413  Salm,  E.,  Die  Bestimmung  des  H+-Gehaltes  einer  Losung  mit 
Hilfe  von  Indikatoren,  Zeitschr.  f.  Electrochem.,  1904,  vol.   10,  pp. 
341-346. 

414  Salm,    E.,    Kolorimetrische    Affinitatsmessungen,    Zeitsehr.    f 
Eleetrochem.,  1906,  vol.  12,  pp.  99-101. 

415  Salm,  E.,   Studie  iiber  Indikatoren,  Zeitschr.   f.  phys.   Chem., 
1906,  vol.  57,  pp.  471-501. 

416  Salm,  E.,  Messungen  der  Affinitatsgrossen  organiseher  Sauren 
mit  Hilfe  von  Indikatoren,  Zeitsehr.  f.  phys.  Chem.,  1908,  vol.   63, 
pp.  83-108. 

417  Salm,  E.,  and  Friedenthal,  H.,  Zur  Kenntnis  der  acidimetrischen 
und  alkalimetrischen  Indikatoren,  Zeitschr.  f.  Electrochem.,  1907,  vol. 
13,  pp.  125-130. 

418  Scatchard,  G.,  and  Bogert,  M.  T.,  A  new  and  very  sensitive 
indicator  for  acidimetry  and  alkalimetry  and  for  determining  hydro- 
gen ion  concentrations  between  the  limits  of  6  and  8  on  the  Sorensen 
scale,  Science,  n.s.,  1916,  vol.  43,  p.  722. 

419  Sorensen,  S.  P.  L.,  and  Palitzsch,  S.,  Sur  un  indicateur  nouveau, 
o-naphtolphtaleine,   ayant   un   virage   au   voisinage   du   point   neutre, 
C.-E.  Lab.,  Carlsberg,  1910,  vol.  9,  pp.  1-7. 

420  Sorensen,  S.  P.  L.,  and  Palitzsch,  S.,  Ueber  den  ' '  Salzfehler ' ' 
bei  der  colorimetrischen  Messung  der  Wasserstoffionenkonzentration 
des  Meerwassers,  Biochem.  Zeitsch.,  1913,  vol.  51,  pp.  307-313. 


Schmidt-Hoagland:  Table  of  PH,  H+  cmd  OR-  Values     67 

421  Stieglitz,  J.,  The  theories  of  indicators,  Jour.  Am.  Chem.  Soc., 
1903,  vol.  25,  pp.  1112-1127. 

422  Thiel,  A.,  Der  Stand  der  Indikatorenfrage,  Sammlung  chem.  u. 
chem.-tech.  Vortrage,  1911,  vol.  16,  pp.  307-422. 

423  Tizard,  H.  T.,  The  colour  changes  of  methyl-orange  and  methyl- 
red   in  acid   solution,  Jour.   Chem.   Soc.,  London,   1910,  vol.   97,  pp. 
2477-2490. 

424  Tizard,  H.  T.,  The  hydrolysis  of  aniline  salts  measured  colori- 
metrically,  Jour.  Chem.  Soc.,  London,  1910,  vol.  97,  pp.  2490-2495. 

425  Walbum,  L.  E.,  Ueber  die  Verwendung  von  Eotkohlauszug  als 
Indikator    bei    der    colorimetrischen    Messung    der    Wasserstoffionen- 
konzentration,  Biochem.  Zeitschr.,  1913,  vol.  48,  pp.  291-296. 

426  Walburn,  L.  E.,  Sur  1'emploi  de  1'extrait  de  choux  rouge  comme 
indicateur  dans  la  mesure  colorimetrique  de  la  concentration  des  ions 
hydrogene,  C.-E.  Lab.,  Carlsberg,  1911,  vol.  10,  pp.  227-232. 

427  Walpole,  G.  S.,  Chart  presentation  on  recent  work  on  indicators, 
Biochem.  Jour.,  1910,  vol.  5,  pp.  207-214. 

428  Wegsoheider,  K.,  Ueber  den  Farbenumschlag  des  phenolphtha- 
leins,  Zeitschr.  f.  Eleetrochem.,  1908,  vol.  14,  pp.  510-512. 


ADDENDA 

429  Baker,  J.  C.,  and  Van  Slyke,  L.  L.,  A  method  for  making  elec- 
trometric  titrations  of  solutions  containing  protein,  Jour.  Biol.  Chem., 
1918,  vol.  35,  pp.  137-145. 

430  Barnett,  G.  D.,  and  Chapman,  H.  S.,  Colorimetric  determination 
of  reaction  of  bacteriologic  mediums  and  other  fluids,   Jour.   Amer. 
Med.  Assoc.,  1918,  vol.  70,  pp.  1062-1063. 

431  de  Corral  y  Garcia,  J.  M.,  La  reaccion  actual  de  la  sangre  y 
su  determinacion  electrometrica.     Tesis  de  doctorado,  Universidad  de 
Madrid,  Valladolid,  1914,  pp.  1-162. 

432  Crozier,   W.   J.,   On   indicators   in   animal   tissues,   Jour.    Biol. 
Chem.,  1918,  vol.  35,  pp.  455-460. 

433  Cullen,  G.  E.,  and  Austin,  J.  H.,  Hydrogen  ion  concentrations 
of  various  indicator  end-points  in  dilute  hydochlorite  solutions,  Jour. 
Biol.  Chem.,  1918,  vol.  34,  pp.  553-568. 

434  Evans,  A.  C.,  A  study  of  the  streptococci  concerned  in  cheese 
ripening,  Jour.  Agri.  Bes.,  1918,  vol.  13,  pp.  235-252. 

435  Evans,  A.  C.,  Bacterial  flora  of  Eoquef  ort  cheese,  Jour.  Agric. 
Ees.,  1917,  vol.  13,  pp.  225-233. 

436  Fred,  E.  B.,  and  Loomis,  N.  E.,  The  influence  of  hydrogen-ion 
concentration,  of  the  medium  on  the  reproduction  of  alfalfa  bacteria. 
Jour.  Bact.,  1917,  vol.  2,  pp.  629-633. 

43T  Gainey,  P.  L.,  Soil  reaction  and  the  growth   of  azotobacter, 
Jour.  Agric.  Ees.,  1918,  vol.  14,  pp.  265-271. 

438  Gainey,  P.  L.,  Soil  reaction  and  the  presence  of  azotobacter, 
Science,  n.s.,  1918,  vol.  48,  pp.  139-140. 

439  Gillespie,  L.  J.,  Correlation  of  H-ion  exponent  and  occurrence 
of  bacteria  in  soil,  Science,  n.s.,  1918,  vol.  48,  pp.  393-394. 

440  Gillespie,  L.  J.,  and  Wise,  L.  E.,  Action  of  neutral  salts  on 
humus  and   other   experiments   on   soil   acidity,   Jour.    Amer.    Chem. 
Soc.,  1918,  vol.  40,  pp.  796-813. 


68     University  of  California  Publications  in  Physiology     [VOL.  5 

441  Gillespie,  L.  J.,  The  growth   of   the  potato   scab   organism   at 
various   hydrogen   ion   concentrations   as   related   to   the   comparative 
freedom  of  acid   soils   from  the  potato   scab,  Phytopathology,   1918, 
vol.  8,  pp.  257-269. 

442  Goldberger,  J.,  The  change  in  the  hydrogen-ion  concentration 
of  muscle  during  work,  Biochem.  Zeitschr.,  1917,  vol.  84,  pp.  201-209, 
after  Chem.  Abs.,  1918,  vol.  12,  p.  1482. 

443  Haas,  A.  E.  C.,  On  the  preparation  of  ovalbumin  and  its  refrac- 
tive indices  in  solution,  Jour.  Biol.  Chem.,  1918,  vol.  35,  pp.  119-125. 

444  Hasselbalch,  K.  A.,  The  reduced  and  the  regulated  ' '  hydrogen 
figure"  of  the  blood,  Biochem.  Zeitschr.,  1916,  vol.  74,  pp.  56-62,  via 
Physiol.  Abs.,  1916,  vol.  1,  p.  252. 

445  Hoagland,  D.  E.,  Studies  on  the  relation  of  the  nutrient  solu- 
tion to  the  composition  and  reaction  of  the   cell  sap   of  the   barley 
plant,  Botanical  Gazette   (in  press). 

446  Hoagland,  D.  E.,  The  relation  of  the  plant  to  the  reaction  of 
the  nutrient  solution,  Science,  n.s.,  1918,  vol.  48,  pp.  422-425. 

447  Hoagland,  D.  E.,  and  Christie,  A.  W.,  The  chemical  effects  of 
CaO  and  CaCo3  on  the  soil,  Soil  Science,  1918,  vol.  5,  pp.  379-382. 

448  Hober,   E.,   Die   Gaskettenmethode   zur   Bestimmung   der   Blut- 
reaktion,  Deut.  med.  Woch.,  1917,  vol.  43,  pp.  551-552,  via  Physiol. 
Abs.,  1918,  vol.  2,  p.  604. 

449  Homer,  A.,  A  note  on  the  use  of  indicators  for  the  colorimetric 
determination   of   the   hydrogen-ion   concentration   of   sera,   Biochem. 
Jour.,  1917,  vol.  11,  pp.  283-291. 

450  Kligler,  I.  J.,  The  effect  of  hydrogen-ion  concentration  on  the 
production  of  precipitates  in  a  solution  of  peptone  and  its  relation 
to  the  nutritive  value  of  media,  Jour.  Bact.,  1917,  vol.  2,  pp.  351-353. 

451  Meacham,  M.  E.,  The  hydrogen-ion  concentration  necessary  to 
inhibit  growth  of  four  wood  destroying  insects,   Science,   n.s.,   1918, 
vol.  48,  pp.  499-500. 

452  Noyes,  A.  A.,  and  Chow,  M.,   The  potentials   of  the  bismuth- 
bismuthoxychloride   and   the   copper-cuprouschloride   electrodes,   Jour. 
Amer.  Chem.  Soc.,  1918,  vol.  40,  pp.  739-763. 

453  Osterhout,  W.   J.   V.,   The   determination  of   buffer   effects   in 
measuring  respiration,  Jour.  Biol.  Chem.,  1918,  vol.  35,  pp.  237-240. 

454  Osterhout,  W.  J.  V.,  A  method  of  studying  respiration.     Jour. 
Gen.  Phys.,  1918,  vol.  1,  pp.  17-22. 

455  Osterhout,  W.  J.  V.,  and  Haas,  A.  E.  C.,  On  the  dynamics  of 
photo-synthesis,  Jour.  Gen.  Physiol.,  1918,  vol.  1,  pp.  1-16. 

456  Eobertson,   T.   B.,   Ueber   die   verbindungen   der   Proteine   mit 
anorganischen    Substanzen   und   ihre    Bedeutung   fiir   die   Lebensvor- 
gange,  Ergeb.  der  Physiol.,  1910,  vol.  10,  pp.  216-361. 

457  Sherman,  H.  C.,  Thomas,  A.  W.,  and  Baldwin,  M.  E.,  Influence 
of   hydrogen-ion   concentration   upon   the    enzymie   activity   of   three 
typical  amylases,  Proc.  Soc.  Exp.  Biol.  and  Med.,  1918,  vol.  16,  pp. 
17-18. 

458  Truog,  E.,  Soil  acidity:  I,  Its  relation  to  the  growth  of  plants, 
Soil  Science,  1918,  vol.  5,  pp.  169-195. 

459  gzili,  A.,  The  reaction  of  human  milk,  Biochem.  Zeitschr.,  1917, 
vol.  84,  pp.  194-200,  quoted  after  Chem.  Abs.,  1918,  vol.  12,  p.  1482. 

460  Van  Slyke,  L.  L.,  and  Baker,  J.  G.,  Free  lactic  acid  in  sour 
milk,  Jour.  Biol.  Chem.,  1918,  vol.  35,  pp.  147-178. 


1919]     Schmidt-Hoagland:  Table  of  PH,  H+  and  OH-  Values     69 

461  Clark,   W.    M.,    The   acid   production    of    Bacillus    Bulgaricus. 
Abstr.  Bact.  Proc.,  1917,  vol.  1,  p.  59. 

462  Cullen,  G.  E.,  and  Chesney,  A.  M.,  Note  on  the  production  of 
acid  by  pneumococci.    Jour.  Exp.  Med.,  1918,  vol.  28,  pp.  289-296. 

463  Dernby,  K.  G.,  and  Avery,  O.  T.,  Optimum  hydrogen-ion  con- 
centration for  the  growth  of  pneumococcus.     Jour.  Exp.  Med.,  1918, 
vol.  28,  pp.  345-357. 

464  Gillespie,  L.  J.,  and  Hurst,  L.  A.,  Hydrogen-ion  concentration 
— soil  type — common  potato   scab.      Soil   Science,   1918,   vol.    6,   pp. 
219-236. 

4G5  Eice,  F.  E.,  and  Osugi,  S.,  The  inversion  of  cane  sugar  by  soils 
and  allied  substances  and  the  nature  of  soil  acidity,  Soil  Science, 
1918,  vol.  5,  pp.  333-358. 

466  Toole,  E.  H.,  and  Tottingham,  W.  E.,  The  influence  of  certain 
added  solids .  upon  the  composition  and  efficiency  of  Knop  's  nutrient 
solution,  Amer.  Jour.  Bot.,  1918,  vol.  5,  pp.  452-461. 

467  Waksman,  S.  A.,  The  occurrence  of  azotobacter  in  cranberry 
soils,  Science,  n.s.,  1918,  vol.  48,  pp.  653-654. 

NOTE.— The  bibliography  has  been  brought  up  to  date  of  publication. 


UNIVEESITY  OF  CALIFORNIA  PUBLICATIONS— (Continued) 

3.  Can  the  Cerebral  Cortex  be  Stimulated  Chemically? .   (Preliminary 

communication),  by  S.  S.  Maxwell.    Pp.  17-19.    February,  1906 06 

4.  The  Control  of  Galvanotropism  in  Paramecium   by  Chemical  Sub- 

stances, by  Frank  W.  Bancroft.    Pp.  21-23.    March,  1906 10 

5.  The  Toxicity  of  Atmospheric  Oxygen  for  the  Eggs  of  the  Sea-urchin 

(Strfngylocentrotui   purpuratvs)    after   the    Process    of   Membrane 
Formation,  by  Jacques  Loeb.    Pp.  SS-S7.    March,  1906. 

6.  On  the  Necessity  of  the  Presence  of  Free  Oxygen  in  the  Hypertonic 

Sea-water   for   the   Production   of   Artificial   Parthenogenesis,   by 
Jacques  Loeb.     Pp.  39-47.    March,  1906. 
Nos,  6  and  6  in  one  cover 18 

7.  On  the  Counteraction  of  the  Toxic  Effect  of  Hypertonic  Solutions 

upon  the  Fertilized  and  Unfertilized  Egg  of  the  Sea-urchin  by  Lack 

of  Oxygen,  by  Jacques  Loeb.    Pp.  49-56.    April,  1906 .05 

8.  On  the  Production  of  a  Fertilization  Membrane  in  the  Egg  of  the 

Sea-urchin  with  the  Blood  of  Certain  Gephyrean  Worms   (a  pre- 
liminary note),  by  Jacques  Loeb.    Pp.  57-58.    March,  1907 „.      .05 

9.  Note  on  the  Synthesis  of  a  Protein  through  the  Action  of  Pepsin 

(preliminary    communication),    by   T.    Erailsford    Robertson.      Pp. 
59-60.     April.  1507 .05 

10.  The  Chemical  Character  of  the  Process  of  Fertilization,  and  ita  Bear- 

ing upon  the  Theory  of  Life-Phenomena,  by  Jacques  Loeb.     Pp. 
61-80.     September,  1907 " , 25 

11.  A  New  Proof  of  the  Permeability  of  Cells  for  Salts  or  Ions  (a  pre- 

liminary communication),  by  Jacques  Loeb.     Pp.  81-86.     January, 

1908    „.       .05 

12.  The  Origin  of  two  new  Retrogressive  Varieties  by  one  Mutation  in 

Mice,  by  Arend  L.  Hagedoorn.    Pp.  87-90.    September,  1908 „      .05 

IS.  On  Synthesis  of  Parunuelein  through  the  Agency  of  Popsin  and  Chemi- 
cal Mechanics  of  Hydrolysis  and  Synthesis  of  Proteins  through  tha 
Agency  of  Enzymes,  by  T.  B.  Robertson.  Pp.  91-94.  Decembar, 
1908  _ 05 

14.  The  Inheritance  of  Yellow  Color  in  Rodents,  by  Arend  L.  Hagedoorn. 

Pp.  95*99.     March,  1909 06 

15.  Table  of  H+  and  OH-  Concentrations  corresponding  to  Electromotive 

Forces  determined  in  Gas-chain  measurements,  by  0.  L.  A.  Schmidt. 

Pp.  101-113.     September,  1909 10 

16.  The  Proteins,  by  T.  Brailsford  Robertson.    Pp.  115-194.    October,  1910  $1.00 

17.  Further  Proof  of  the  Identity  of  Heliotropism  in  Animals  and  Plants, 

by  Jacques  Loeb  and  S.  S.  Maxwell.     Pp.  195-197.     January,  1910      .05 

Vol.4.      1.  Experiments  on  the  Function  of  the  Internal  Ear,  by  S.  S.  Maxwell. 

Pp.  1-4.    September,  1910  05 

2.  On  the  Rise  of  Temperature  in  Rabbits,  Caused  by  the  Injection  of  Salt 

Solutions,  by  Theo.  C.  Burnett.    Pp.  5-7.    September,  1910  05 

3.  A  Biochemical  Conception  of  Dominance,  by  A.  R.  Moore.    Pp.  9-15. 

September,  1910  _ 05 

4.  Galvanotropic  Orientation  in  Gonium  pectorale,  by  A.  R.  Moore  and  T. 

H.  Goodspeed.    Pp.  17-23.    May,  1911 .05 

5.  On  a  Possible  Source  of  the  Biological  Individuality  of  the  Tissues  and 

Tissue-fluids  of  Animal  Species,  by  T.  Brailsford  Robertson.     Pp. 
25-30.    May,  1911 05 

6.  Some  Factors  Influencing  the  Quantitative  Determination  of  Gliadin, 

by  J.  E.  Greaves.    Pp.  31-74.    August,  1911  40 

7.  Errors  of  Refraction  Occurring  in  the  Students  of  the  University  of 

California,  by  Theo.  0.  Burnett.    Pp.  75-77.    August,  1911 05 

8.  On  the  Cytolytic  Action  of  Ox-Blood  Serum  upon  Sea-Urchin  Eggs, 

and  Its  Inhibition  by  Proteins  (Preliminary  communication),  by  T. 

Brailsford  Robertson.     Pp.  79-88.     February,  1912 10 

9.  On  the  Nature  of  the  Cortical  Layer  in  Sea  Urchin  Eggs,  by  A.  R, 

Moore.    Pp.  89-90.    March,  1912. 

10.  On  the  Nature  of  the  Sensitization  of  Sea  Urchin  Eggs  by  Strontium 
Chloride,  by  A.  R.  Moore.  Pp.  91-93.  March,  1912. 

Nos.  9  and  10  in  one  cover 05 

11.  On  the  Isolation  of  Ob'cytase,  the  Fertilizing  and  Cytolyzing  Substance 
in  Mammalian  Blood  Sera,  by  T.  Brailsford  Robertson.  Pp.  95-102. 
March,  1912. 


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